# Co O2 Co2 Equilibrium Constant

For the reaction given below at 700°C, Kc = 0. 10 mol/L for PCl 3. Compared to the original system, the rates of the forward and reverse reactions of the new equilibrium. increasing the temperature 13. Definition of equilibrium constant Kp for gas phase reactions, and how to calculate Kp from Kc. Reactions don't stop when they come to equilibrium. 0908 moles of H 2, 0. adding NO(g) C. of products conc. 0 M, calculate the concentration of CO. Carbon dioxide in water equilibrium. 5 × 10 −3 M. Equilibrium 8 Pressure Equilibrium Constants K is the general symbol for equilibrium constant K c is the equilibrium constant defined by concentrations K p is the equilibrium constant defined by partial pressures Below shows how K c and K p are defined for same reaction For reaction: N 2 (g) + 3H 2 (g) 2NH 3 (g) K c = [NH 3] 2 / [N 2] [H 2] 3 K. 17  1031 C) 2. We use the chemical equilibrium to determine the extent and drive of the chemical reaction. 2CO + O2 = 2CO2. CO2(g) + C(graphite) ⇌ 2 CO(g)-The equilibrium constant will increase. 2H2O + CO2 ---> 3/2O2 + CH3OH 2. So the O2s are now balanced as well. When carbon dioxide dissolves in water, it exists in chemical equilibrium with carbonic acid: + ↽ − − ⇀ The hydration equilibrium constant at 25 °C is called K h, which in the case of carbonic acid is [H 2 CO 3]/[CO 2] ≈ 1. (b) Oxygen gas oxidizes gaseous ammonia to gaseous nitrogen monoxide; water vapor is the other product. 8 KJ/mol -25. Numerade Educator 02:21. What is the equilibrium partial pressure of oxygen in a sample at 1000 °C for which the initial pressure of CO 2 was 1. For a reaction made up of two or more steps, the equilibrium constant for the net. 50 moles of N 2 gas is mixed with 0. 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following 11) reaction:CO (g) + H2O (g) CO2 (g) + H2 (g)In an experiment, 0. At this temperature, K c equals 1. The point of intercept of three lines represent CO-CO2-O2 equilibrium when CO and CO 2 are at 1 atmosphere pressures. CHEMICAL EQUILIBRIUM. types in this section: rate constants based on equilibrium constants, and treatment of OH + O2. 00 L reaction vessel were present at equilibrium. Keq: Equilibrium Constant. The top arrow points to the right. For the gas-phase reaction. 2 The constituents of the mixture are ideal gases. 00 moles each of H2(g) and CO2(g) are placed in a 1. First, be sure to count all of C and O atoms on each side of the chemical equation. 16 mol of CO remaining. Problem Methane, ethyne, and hydrogen form the following equilibrium mixture. 47) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. 27) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. 1k points) equilibrium. In the absence of a catalyst, the equilibrium is reached quite slowly. The value of log 10 (K eq) for the reaction as a function of temperature in Kelvin (valid between 500– 2200 K) is approximately: log10(Keq). There is equilibrium between the molecules in the gaseous state and the molecules dissolved in the liquid under pressure i. (d) The equilibrium constant for the reverse reaction, K′, is the reciprocal of K. equilibrium constants and le chatelier's principle This page looks at the relationship between equilibrium constants and Le Chatelier's Principle. Answer to: For the reaction 2CO(g)+O2(g)<-->2CO2(g), the value of K at a certain temperature is 1300. Similarly, if you decreas. 0 L, to get the equilibrium concentration of CO2. The number of moles of H2, S2, and H2S present at the equilibrium for the reaction are 2. Keq: Equilibrium Constant. Thus efficiency of CO2 removal from gas depends only on kinetics (contact surface and time) in this case. The equilibrium constant K p = 2. The resultant fitted values of the Adair constants, al, a2, and a3, were similar to those obtained when K4 was allowed to vary, and the fits. Write the equilibrium equation for each of the following reactions: a) 2 SO2(g) + O2(g) 2 SO3(g) b) 2 SO3(g) 2 SO2(g) + O2(g) The following equilibrium concentrations were measured at 800 K: [SO2] = 3. 35 mol of CO and 0. [CH3OH][H2O]/ [CO2][H2]^3 x [CO2][H2]/ [CO][H2O] x [CO]^2 / [C]^2[O2] = [CH3OH][CO] / [C]^2[H2]^2[O2] 1. The equilibrium constant for the following reaction is 600(C is 4. Compared to the original system, the rates of the forward and reverse reactions of the new equilibrium. 4 atm due to a much higher equilibrium conversion of 0. 7×10 −3 in pure water and ≈ 1. The cooperativity of O 2 binding and the effects of nonstandard physiological conditions are established in this model by considering the equilibrium constant for the reaction of O 2 with an Hm-NH 2 chain as a suitable function of P O 2, P CO 2, pH, [2,3-DPG] and T involving six adjustable parameters (see Eq. The reaction quotient Ω=Q/K numerically describes if the reaction can occur. -The equilibrium constant will decrease. The supply of CO 2 and O 2 in the environment is unlimited. At this temperature, Kc equals 1. 352 mol/L, and [H2O] = 0. The reversibility of this reaction was discovered by Deville in 1864, and its study receives renewed interest in view of recent developments in the theory of the combustion of carbon in oxygen to which reference has already been made. As a result, the pH of the blood is lowered, causing acidosis. Carbon dioxide in water equilibrium. Keq = (H2O) (CO) / (H2) (CO2) Pretty sure it's called it's Boiling Point. , CO 2 (gas) ⇌CO 2(in solution) This equilibrium is governed by. 00-2x 2x x Therefore the [O2] = 5. a)i) Calculate the amounts, in moles, of methane, steam and hydrogen in the equilibrium mixture. P_CO = Pa0*(1-Xeq) P_H2O = Pa0*(1-Xeq) P_H2 = Pa0*Xeq P_CO2 = Pa0*Xeq P_CO = 2. 2NH3(g)+CO2(g), which at 300K, the equilibrium constant, Kp is 0. At 100°C the equilibrium constant for the reaction COCl 2 (g) CO(g) + Cl 2 (g) has the value of K c = 2. Anyway, above 750 o C, CO is predominant and stable. 0 M and the concentration of O2 is 9. 16 mol of CO remaining. Generally omit the. 7 × 10-2 M, and CO2 was measured to be 1. At constant temperature, for Le Chatêlier purposes, Adding $\ce{CO}$ produces that it react with $\ce{O2}$ to produce more $\ce{CO2}$ to counteract the effect of the applied change and a new equilibrium is established. 20 mol of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C (s) + CO2 (g) <--> 2CO (g) Under these conditions, the average molar mass of the gas was 35 g/mol. So for the first example let's say we have calcium carbonate solid, in equilibrium with calcium oxide solid and carbon dioxide gas. Consider the following reactions I. 86 moles of O 2 gas in a 2. We adopted a larger uncertainty. The equilibrium mixture contained 0. Equilibrium constant: Here K. Consider the reaction: C(s) + O2(g)---> CO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below: a. Assume that one has an equilibrium mixture of these substances. 000 L vessel. 648 mol/L, [H2] = 0. 000355 Atmosphere. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. Balancing problem is now solved. Increase in concentration => increase in rate Decrease in concentration => decrease in rate If you increase the concentration of the reactants, the forward reaction rate increases and the equillibrium shifts to the right. 7 J/K The equilibrium constant for this reaction at 344 K is: A) 1. 71 x 10^27 which is the equilibrium constant for: C + H2 + 1/2O2 ===⇒ 1/2CH3OH + 1/2CO. For which one of the following reactions does Kp equal Kc? (Points : 10) 1. Having equilibrium data for sodium bicarbonate could be of significant interest due to its practicality as a candidate sorbent used in the growing industry of CO 2 capture. The equilibrium constant (Kc) for the following reaction is 6. Chapter 13 Fundamental Equilibrium Concepts Figure 13. CO(g)+H2O(l)⇌H2CO3(aq) This reaction is not balanced, so an equilibrium expression cannot be written properly. Calculate [CO2] at equilibrium when [CO] = for Teachers for Schools for Working Scholars. The dissociation of carbon dioxide in the carbon monoxide-oxygen flame has been investigated by Haber and Rossignol, by the method of Deville, and these authors find that the value of the equilibrium constant K in the equation K = [CO 2]/[CO]×[O 2] ½. Consider the following equilibrium system: O 2(g) + 2HF (g) ⇌ OF 2(g) H = +318 kJ/mol If the temperature of the system is increased, A. With atmospheric CO2 at 400 ppm, the mass of CO2 in the atmosphere is 2 E15 kg Therefore, if ALL the CO2 in the atmosphere were to be instantly sucked into the ocean (and evenly mixed), that would result in an increase in the concentration of CO2 in seawater of about 1. Determine the equilibrium constant KP at this temperature. Section 5- Carbonate Chemistry CASE 1 CO 2 - H 2 O open system Aqueous carbon dioxide reacts to form carbonic acid via the following reaction: 2 0. 500 mole of carbon monoxide and 0. Removing $\ce{CO2}$ produce that $\ce{CO}$ react with $\ce{O2}$ to produce more $\ce{CO2}$. 00×10−13 Express your answer numerically. D (g) + 2 CB (s) 4. 00 a) Find the equilibrium. The K eq was defined earlier in terms of concentrations. The comparison of equilibrium CO 2 solubility and second order reaction rate constant is revealed in Table 9. [CO2] = ___M [O2]=___M [CO]=___M I honestly have tried this so many times, I just don't get it! Could you please work it out and provide the answer! I know some people already asked. 00159 2 (aq)32 2 3 -2. some examples: If CO 2 concentration increases in the atmosphere because of an increased rate of outgassing, global temperature will rise. SbCl5(g) m SbCl3(g) + Cl2(g) b. CO (g) + H2O (g)-----CO2 (g) + H2 (g) if a 10L vessel has 2. The equilibrium constant for reaction (1) below is K. 2 CO2(g) 2 CO(g) + O2(g) If 1. Consider the following equilibrium: H 2 O (g) + CO (g) H 2(g) + CO 2(g) At high temperature, H 2 O and CO are placed in a closed container. #color(blue)(aA + bB rightleftharpoons cC + dD)" "#, where. 0010 M CO2 and 0. 8 KJ/mol Estimate The Value Of The Equilibrium Constant At 625 K For The Following Reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g)2 CO(g) + O2(g) ⇌ 2 CO2(g). Problem: Consider this reaction. ) CO (g) + 1/2 O2 (g) CO. 2803 10 T 1. The equilibrium constant for the reaction: N2(g) + 3H2(g) ⇄ 2NH3(g), is Kc = 3. (a) Carbon monoxide gas reduces nitrogen monoxide gas to gaseous nitrogen; carbon dioxide gas is the other product. The equilibrium equation for the formation of ammonia is: N 2(g) + 3H 2(g) 2NH 3(g) In an equilibrium mixture at 200 °C, the concentrations were found to be as follows: [N 2] = 2. 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0. The number of moles of H2, S2, and H2S present at the equilibrium for the reaction are 2. Compared to the original system, the rates of the forward and reverse reactions of the new equilibrium. What are the equilibrium partial pressures of CO and CO2 at 1050 K if the initial partial pressures are: p CO= 1. An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. 1 × 10-2 M, the concentration of O2 was measured to be 1. CO2, H2O, O2, and N2 For rich mixtures CO also exists in the products and at high temperatures the molecules dissociate to form H, O, OH, NO via the following reactions: The opposite direction reactions are also possible At equilibrium the rate of the forward reaction equals the rate of the backward reaction. ) C(s) + O2(g) <----->CO2(g) Ka. equilibrium is a state in which. Carbon dioxide in water equilibrium. Consider the following reactions and approximate free energy changes: Hgb + O2 —> HgbO2 ∆G⁰ = -70 kJ Hgb + CO —> HgbCO ∆G⁰ = -80 kJ Using these data, estimate the equilibrium constant value at …. 2NH3(g)+CO2(g), which at 300K, the equilibrium constant, Kp is 0. [H 2], [CO], [CH 4], and [HO] are constant with time rate of CO + 3 H 2! CH 4 + HO is the same as the rate of CH 4 + H 2O ! CO + 3 H 2 Position of Chemical Equilibrium the equilibrium position refers to the relative amounts of reactants and products in the system at the point of equilibrium a reaction with an equilibrium position that favors. Get the detailed answer: 73. 2 CO(g) + O2(g) m 2 CO2(g)" is broken down into a number of easy to follow steps, and 44 words. N 2(g) + 3H 2(g) <-----> 2NH 3(g) A. The model solutions describe that, at standard physiological conditions, the hemoglobin is about 97. 937 * 10³ As K > 1 the equilibrium favours the products. 0 mol H2, and 0. The system was prepared with [NH3] = [O2] = 3. 1600 mol of H2O is placed in a 2. CH40S Chemical Equilibrium Unit Review Part A: Multiple Choice 1. That is, the indicated reaction will be less complete at higher temperatures. Rate constant expression from the evaluation of Tsang and Hampson (1986), taken from an earlier review by Baulch. 1) Gas dissolution. 00×10−13 Express your answer numerically. 7 x 10-2 M [NH3] = 1. 2803 10 T 1. be determined by measuring the equilibrium vapor pressure as a function of temperature. Taking the derivative of the Gibbs energy with respect to the extent of reaction gives the minimum Gibbs energy at the equilibrium extent. Calculating Equilibrium Constants Calculating Equilibrium Constants Phosphorous Problem 3(a) Carbon dioxide decomposes at elevated temperatures to carbon monoxide and oxygen: 2CO2(g) 2CO(g) + O2(g) At 3000 K, 2. For example, if the temperature of a mass of CO2 gas in a vessel is increased sufficiently, some of the CO2 molecules dissociates into CO and O2 molecules. 2 O3(g) <-> 3 O2(g) 3. A system at equilibrium is in a state of dynamic balance, with forward and reverse reactions taking place at equal rates. 17  1031 C) 2. 74 x 10 46 B) 1. At constant temperature, for Le Chatêlier purposes, Adding $\ce{CO}$ produces that it react with $\ce{O2}$ to produce more $\ce{CO2}$ to counteract the effect of the applied change and a new equilibrium is established. View Test Prep - quiz. At this temperature, K c equals 1. 57(mol(CO, 0. INFO - Refractive index database Shelf. 2) Carbonic acid formation. At 850 degrees C and 1 atm pressure, a gaseous mixture of carbon monoxide and carbon dioxide in equilibrium with solid carbon is 90. 56 T (cal)) R T ln = -135194 + (41. 6) Typically, either the forward or backward reaction is defined in terms of a bimolecular or. 7252 Compare the equilibrium constants. Hi! Can somebody please help me? At 1200 K, the approximate temperature of vehicle exhaust gases, Kp for the reaction 2CO2(g) -> <- 2CO(g) + O2(g) is about 1 E-13. From the reaction among these three species: G = - R T ln P P P CO CO O 2 2 2 2 G = R T ln P O 2. H2 (g) + I2 (g) ↔ 2 HI (g). The O2 and CO2 content in whole blood are also calculated here from the gas solubilities, hematocrits, and the new formulas for  S_{{{\text{HbO}}_{ 2. The bottom arrow points to the left. CH40S Chemical Equilibrium Unit Review Part A: Multiple Choice 1. 45 mol of carbon monoxide and 2. 2CO + O2 = 2CO2. 0 M, calculate the concentration of CO. Question: A Reaction Has An Equilibrium Constant Of 7. The following equilibrium is observed: Co(H 2 O) 62+ (aq) + 4 Cl - (aq) <=> CoCl 42- (aq) + 6 H 2 O(g) The Co(H 2 O) 62+ complex is pink, and the CoCl 42- complex is blue. (1) The equilibrium constant, K, is much stronger in haemoglobin-carbon monoxide reaction compared to the haemoglobin-oxygen reaction which means that the haemoglobin puts priority on carbon monoxide bonds, therefore the haemoglobin that has bonded with carbon monoxide is no longer available for oxygen. Carbonate equilibrium constant in water: Q = [CO. We use the chemical equilibrium to determine the extent and drive of the chemical reaction. K' = K 1 x K 2. P_CO = Pa0*(1-Xeq) P_H2O = Pa0*(1-Xeq) P_H2 = Pa0*Xeq P_CO2 = Pa0*Xeq P_CO = 2. [CH3OH][H2O]/ [CO2][H2]^3 x [CO2][H2]/ [CO][H2O] x [CO]^2 / [C]^2[O2] = [CH3OH][CO] / [C]^2[H2]^2[O2] 1. 19 mol of CO remaining. When you put these numbers into the equation, K is found to be: K = 0. 40 10-33 18. 35 mol/L, and [O. 5 M, and Kc = 2. The reaction CO(g)+H2O(g)-->CO2(g)+H2(g) has the equilibrium constant kp of 23. Equilibrium constant is a number that expresses the relationship between the amounts of products and reactants present at equilibrium for a reversible chemical reaction at a given temperature. 7 J/K The equilibrium constant for this reaction at 344 K is: A) 1. Analysis Assuming N2 to remain as an inert gas, the stoichiometric and actual reactions can be written asStoichiometric: CO + 1 O 2 ⇔ CO 2 (thus ν. 00-L reaction vessel. , different ion concentrations, pH and/or alkalinity) with different levels of CO2 , N2 and/or O2 in the system. However, the oceans are no longer able to absorb the increased concentration of CO 2 in the atmosphere without changes to the acidity levels. 4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). 20 at 600°C. At 855 K, The Equilibrium Constant Is 0. 5, calculate Kc for Reaction 2 CO2(g)␣CO(g) + 1/2O2(g) how do i calculate kc?. If you're seeing this message, it means we're having trouble loading external resources on our website. Stempien et al. Multiple Choice 48. Chemical Equilibrium. In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H 2 O (g) ↔ CO 2 (g) + H 2 (g) In an experiment, 0. Where, ΔG ° is the standard free change of a reaction, value of ΔG ° is -35000 (calculated in part(a)) R = gas constant, value of R is 8. The reversibility of this reaction was discovered by Deville in 1864, and its study receives renewed interest in view of recent developments in the theory of the combustion of carbon in oxygen to which reference has already been made. 502 + 5N2 at 4 atm (e) 2CO + O2 2CO2 at 1 atm. Reaction Information. , CO 2 (gas) ⇌CO 2(in solution) This equilibrium is governed by. The equilibrium constant depends on the initial concentrations. 2 (c) H2O(l)⇌H2O(g)T=60°CKp=0. Consider the reaction 2 CO2 ⇔ 2 CO + O2 obtained after heating 1 kmol CO2 to 3000 K. (c) Derive and use the equation, Kp = Kc (RT)n. 1 mol NaHCO 3. 0092 moles of H 2 O vapor were present in a 2. What is the equilibrium concentration of CO? An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. 54 MPa using an isochoric method. 2CO2 (g) 2CO (g) + O2 (g) DHe = -514 kJ. the concentration of all dissolved CO2 by [H2CO3]. The equilibrium constant {eq}\left( {{K_{\rm{p}}}} \right) {/eq} is a value determined by taking the ratio of partial pressures of all the gaseous products to the partial. Because H 2 O is the only non-condensed phase present, the equilibrium constant is P(H 2 O) 3 = (. The equilibrium constant for reaction (1) below is K. The supply of CO 2 and O 2 in the environment is unlimited. The equilibrium constant {eq}\left( {{K_{\rm{p}}}} \right) {/eq} is a value determined by taking the ratio of partial pressures of all the gaseous products to the partial. [CO] [O2] [CO2] 3. Chemical equilibrium. What are the concentrations of all the substances when the reaction reaches the equilibrium? | EduRev Class 11 Question is disucussed on EduRev Study Group by 251 Class 11 Students. 22 mol of water vapour are combined in a 1. 5 mole of CO2 and 0. CO2(g) + H2(g) ( CO(g) + H2O(g) At equilibrium, [CO2] = 0. Use an ICE table for your calculation. 00 mol CO2 and H2 gas at 588K, what are the concentrations of all species at equilibrium. The CO placed in the vessel is labelled with 14C. At 800°C, the concentration of CO 2 in equilibrium with solid CaCO 3 and CaO is 2. Suppose the equilibrium [PCl3] = equilibrium [Cl2] = x mol dm^-3 then the equilibrium [PCl5] = 0. H2 (g) + I2 (g) ↔ 2 HI (g). org are unblocked. the equilibrium state 01. Hence, the majority of the carbon dioxide is not converted into carbonic acid, remaining as CO 2 molecules. 1Chemical Equilibria 13. 72 atm CO2, and 0. This equilibrium constant example concerns a reaction with a "small" equilibrium constant. 2CO (g) + O2 (g) ⇄ 2CO2 (g) + energy. Increase in concentration => increase in rate Decrease in concentration => decrease in rate If you increase the concentration of the reactants, the forward reaction rate increases and the equillibrium shifts to the right. 4 atm and CO2 p = 0. Generally omit the. Reversible reactions, equilibrium, and the equilibrium constant K. 55% CO by mass. 16-17 16-29E A mixture of CO, O2, and N2 is heated to a high temperature at a constant pressure. 623 Concepts and reason An equilibrium constant for a chemical reaction is a certain value of the reaction at equilibrium state, which depends on the temperature at equilibrium. This section derives the equilibrium constant relationship from the general expression for Gibbs Energy of a mixture developed in Chapter 9. In the system we evaluated, at equilibrium we would expect to find that [O 2 ] eq = [N 2 ] eq = 0. 26 minutes ago At 250°C the equilibrium constant (Kp) for the reaction below is 1. 00159 2 (aq)32 2 3 -2. General Chemistry 3rd ed. 7252 P_CO2 = 2. Assuming that the exhaust gas (total pressure 1 atm) by volume contains 0. The equilibrium constant for reaction (1) below is K. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. Calculate the value of [N2]eq if [H2]eq = 2. At this temperature, Kc equals 1. 00 moles each of H2(g) and CO2(g) are placed in a 1. org are unblocked. Consider the reaction: S (s) + O2 (g) CO2 (g) Ka b. Chemical Equilibrium. What is the equilibrium constant for the following reaction, NH3(g) ⇄ ½ N2(g) + 3/2 H2(g) 2. Definition of equilibrium constant Kp for gas phase reactions, and how to calculate Kp from Kc. At equilibrium, there were 0. Hence, the majority of the carbon dioxide is not converted into carbonic acid. The top arrow points to the right. The following equilibrium is observed: Co(H 2 O) 62+ (aq) + 4 Cl - (aq) <=> CoCl 42- (aq) + 6 H 2 O(g) The Co(H 2 O) 62+ complex is pink, and the CoCl 42- complex is blue. 4 atm and CO2 p = 0. SCH4U Answers to Equilibrium Problems 1. Equilibrium constants are defined in the NASA/JPL database in terms of two parameters, A and B: eq exp , 200 K 300 K B KA T T. 21 Equilibrium constant, Kc for the reaction. 2 CO2(g) <-> 2 CO(g) + O2(g) 2. In an open system, the partial pressure of CO 2 (g) is relatively constant at P(CO 2) = 0. 30 M before they are mixed and when equilibrium is reached, the equilibrium concentration of A2D is 0. At equilibrium,. Knowing the initial concentration values and equilibrium constant we were able to calculate the equilibrium concentrations for N 2, O 2 and NO. If for the NH. 2 CO(g) + O2(g) m 2 CO2(g)" is broken down into a number of easy to follow steps, and 44 words. 0908 moles of H 2, 0. The equilibrium constant for the reaction: N2(g) + 3H2(g) ⇄ 2NH3(g), is Kc = 3. The formation of ammonia is an extremely important reaction worldwide for the production of fertilizers and explosives. Write the chemical equation for the equilibrium. 7 x 10-2 M [NH3] = 1. 0 L sealed ﬂask at. For example, at 550K the equilibrium constant is about 58, and the pressure of H2 is 4. 28x10^23)^2 x (1. 127 M, and [NO2] = 15. Link to: Dissociation of CO2 to CO and O2 Applet Link to: Dissociation of N2 and O2 to NO Applet Previously, the products of combustion were determined assuming that the reaction temperature did not reach greater than 1000 K. The equilibrium constant for the formation of CO2 by the reaction 2CO (g) + O2 (g) ↔ 2 CO2 (g) is 1. 148 mol/L, [CO] = 0. 45 moles each of N2 (g) and O2 (g) are introduced in a container that has a volume of 6. 15 At 700 K, equilibrium constant for the reaction: H2 (g) + I2 (g) ƒ 2HI (g) is 54. 0092 moles of H 2 O vapor were present in a 2. 00 2 Similarly, in the equilibrium between nickel, carbon monoxide and nickel carbonyl (used in the purification of nickel), Ni (s) + 4 CO (g) ⇌ Ni(CO)4 (g), the equilibrium constant is written as ( )⎤⎡Ni CO⎣ 4 ⎦K = c [CO]4 It must be. Use data from Appendix IIB to calculate the equilibrium constants at 25°C for each reaction. The Equilibrium 2CO = CO 2 + C. 00159 2 (aq)32 2 3 -2. Atequilibrium, there were 0. H2 (g) + I2 (g) ↔ 2 HI (g). 00 mol of POCl3 Calculate the Keq for the reaction:. Solids and liquids are not taken into consideration when determining equilibrium constants. 7 x 10-2 M [NH3] = 1. If you're behind a web filter, please make sure that the domains *. Kp = Kc (0. If we raise the temperature we add more heat to this equilibrium reaction. We adopted a larger uncertainty. 00 L tank at 2000 K. If the mixture of CO2, CO, and O2 is in equilibrium, then CO2 molecules are dissociating into CO and O2 at the same rate as CO and O2 molecules are recombining in the proportions required to. The comparison of equilibrium CO 2 solubility and second order reaction rate constant is revealed in Table 9. Keq = [CO]2 [CO2][C] C. Kc for the reaction CO(g) + H2O(g) CO2(g) + H2(g), at 800K is 4. Reversible reactions, equilibrium, and the equilibrium constant K. For absolute carbon control accuracy the Process Factor can be continuously updated based on the carbon potential calculated from a 3 gas (CO, CO2 , CH4 ) ULTRACARB 1000 INFRA RED. What is the equilibrium concentration of CO? An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. Assuming that the exhaust gas (total pressure 1 atm) by volume contains 0. N 2(g) + 3H 2(g) <-----> 2NH 3(g) A. 2 NO2(g) <--> 2 NO(g) + O2(g) The equilibrium constant KP is 158. A mixture of 0. org are unblocked. 20 mol of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C (s) + CO2 (g) <--> 2CO (g) Under these conditions, the average molar mass of the gas was 35 g/mol. Please explain the steps to get the answer! Thanks!!. Hb (aq) + 4CO (g) –> Hb(CO) 4 (aq). b) increase the partial pressure of CO (g) at equilibrium. It is due to the property of pressure being disrupted in this system that causes a sudden decrease of oxygen that cannot be reimbursed. Equilibrium constant is a number that expresses the relationship between the amounts of products and reactants present at equilibrium for a reversible chemical reaction at a given temperature. At equilibrium, there were 0. Also, the pressure of CO2 is given, and therefore, first we solve for Kp and then solve for Kc. As you can see, the equilibrium constant is essentially the ratio of the concentration of the products over the concentration of the reactants to the power of each of their respective coefficients. 2CO (g) + O2 (g) ⇄ 2CO2 (g) + energy. Ethane and steam are fed to a steam cracker at a total pressure of 1 atm and at 1000K at a ratio of 4 mol H2O to 1 mol ethane. [CO] increases and [CO2] decreases D. Reactions don't stop when they come to equilibrium. 20 M and [SO3] = 11. The top arrow points to the right. The bottom arrow points to the left. Calculate the equilibrium partial pressure of CO2. 35  10-5 and 8. 8 2 (aq) CO + HO H CO H CO = 10 CO → = The hydration of carbon dioxide is slow to attain equilibrium below pH 8 in pure systems. At this temperature, Kc equals 1. C (s graphite) + 1 O2 (g) → CO2 (g) Back to reactions list. Subtracting 3/2 from 2 gives us 1/2 O2, which matches with the final equation. 000 moles, [P4]eq = 3. The equilibrium mixture contained 0. Atequilibrium, there were 0. At this temperature, Kc equals 1. 97 H2(g) + CO2(g) <–> H20(g) + CO(g) Kp2 = 0. iv) Raising the temperature would shift the equilibrium to the right. Reversible Reactions and Chemical Equilibrium At high temperatures, carbon dioxide gas decomposes into carbon monoxide and oxygen gas. An equilibrium mixture at 500 K has the following concentrations: [N2] = 3. 0 M and the concentration of O2 is 9. The equilibrium concentration of COBn was 0. C(s) + H2O(g) <-> H2(g) + CO(g) 4. Briefly account for. Practice Quiz Equilibrium AP Chemistry 1. 50 moles of N 2 gas is mixed with 0. 2 CO2(g) <-> 2 CO(g) + O2(g) 2. 2 "The Equilibrium Constant" that the equilibrium constant for the decomposition of CaCO 3 (s) to CaO(s) and CO 2 (g) is K = [CO 2]. The reaction continues until a balance is established between these two processes and an equilibrium condition is reached. Find the value of the equilibrium constant for. Calculate the value of the equilibrium constant, KC, for the reaction. The number of moles of H2, S2, and H2S present at the equilibrium for the reaction are 2. The dissociation of carbon dioxide in the carbon monoxide-oxygen flame has been investigated by Haber and Rossignol, by the method of Deville, and these authors find that the value of the equilibrium constant K in the equation K = [CO 2]/[CO]×[O 2] ½. Gaseous carbon dioxide is partially decomposed according to the equation below. the equilibrium state 01. At 855 K, The Equilibrium Constant Is 0. 4 kPa, amine concentration of 2 mol·L −1 and the second-order reaction constant was determined at 298 K , , , ,. A)increase the partial pressure of O2(g) B)decrease the value of the equilibrium constant C)increase the partial pressure of CO D)decrease the partial pressure of CO2(g) E)increase the value of the equilibrium constant 16) Consider the following reaction at equilibrium. 4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). CO (g) + H2O (g) ⇄ CO2 (g) + H2 (g) Calculate the value of the equilibrium constant. Write the symbolic expression for Kc for: Reaction 1 2CO(g) + O2(g) 2CO2(g) If Kc for reaction 1 is equal to 2. If the equations of reactions are added, the equilibrium constant of the resulting reaction is obtained by multiplying the equilibrium constants of the reactions added. 7 J/K The equilibrium constant for this reaction at 344 K is: A) 1. In the table below are data that show the percent of CO in the equilibrium mixture at two different temperatures. 0 x 10-3 M [O2] = 3. Introduction. The coefficients a , b , c , and d in the chemical equation become exponents in the expression for K eq. The top arrow points to the right.  investigated elementary reactions involved in co-electrolysis, but assumed that only H 2 O contributes to the Nernst equation. The point of intercept of three lines represent CO-CO2-O2 equilibrium when CO and CO 2 are at 1 atmosphere pressures. If you're seeing this message, it means we're having trouble loading external resources on our website. So for the first example let's say we have calcium carbonate solid, in equilibrium with calcium oxide solid and carbon dioxide gas. The Equilibrium 2CO = CO 2 + C. rate is kept low enough that equilibrium will be attained, and analysis of the effluent gas gives the data necessary for calculation of the equilibrium constant. 00 L reaction vessel were present at equilibrium. The top arrow points to the right. 7 Le Châtelier’s Principle • 14. 15 At 700 K, equilibrium constant for the reaction: H2 (g) + I2 (g) ƒ 2HI (g) is 54. Problem: Consider this reaction. Compared to the original system, the rates of the forward and reverse reactions of the new equilibrium. 1000 mol of H2 and 0. At 300 K, Keq is equal to 0. An initial pressure of I. (1992) 156, 443-483 Sodium-Calcium Exchange: Derivation of a State Diagram and Rate Constants from Experimental Data EDWARD A. Find the equilibrium constant from the shift in Gibbs function and verify its value with the entry in Table A. It depends on the ionic strength and temperature and is independent of the concentrations of reactants and products in a solution. At 2300 o C, the equilibrium constant for this reaction is 2. 00 a) Find the equilibrium. Practice Quiz Equilibrium AP Chemistry 1. If one has a mixture that is initially composed of 0. 13) + 1(-393. Calculate [CO2] at equilibrium when [CO] = for Teachers for Schools for Working Scholars. The following equilibrium is observed: Co(H 2 O) 62+ (aq) + 4 Cl - (aq) <=> CoCl 42- (aq) + 6 H 2 O(g) The Co(H 2 O) 62+ complex is pink, and the CoCl 42- complex is blue. 000 moles, [P4]eq = 3. 2 percent CO, 12 percent CO 2, and 3 percent O 2, is the system at equilibrium with respect to the above reaction? Online Text. Did the equilibrium shift favour the formation of reactants or products? A catalyst was added to the system at constant volume and a new equilibrium was established. 3 Relationships between K c and K p Values • 14. 2 CO (g) + O2 (g) <===> 2 CO2 (g) is 1. When carbon dioxide dissolves in water, it exists in chemical equilibrium with carbonic acid: + ↽ − − ⇀ The hydration equilibrium constant at 25 °C is called K h, which in the case of carbonic acid is [H 2 CO 3]/[CO 2] ≈ 1. If the amounts of H + and CO 2 exceed the capacity of hemoglobin, they affect the carbonic acid equilibrium (Equation 10), as predicted by Le Ch; âtelier's Principle or the quantitative treatment in terms of equilibrium constants. 7 J/K The equilibrium constant for this reaction at 344 K is: A) 1. equal to its coefficient in the balanced equation. Justify your prediction. CO2, H2O, O2, and N2 For rich mixtures CO also exists in the products and at high temperatures the molecules dissociate to form H, O, OH, NO via the following reactions: The opposite direction reactions are also possible At equilibrium the rate of the forward reaction equals the rate of the backward reaction. The bottom arrow points to the left. When equilibrium was reached, there was still some C(s) remaining in the container. For a chemical equilibrium, the equilibrium constant is defined as the ratio between the product of the equilibrium concentrations of the products and the product of the equilibrium concentrations of the reactants, all raised to the power of their respective stoichiometric coefficients. 40 x 10^2 x 1. The backward rates are derived from equilibrium constants of reaction and the forward rates as shown in (7) : kbi = kfi Ki (7) In addition, the equilibrium constant of the reaction 2 can be written with that of reac-tion 1, see (8). An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. Full text of "Heats, free energies, and equilibrium constants of some reactions involving O2, H2, H2O, C, CO, CO2, and CH4" See other formats U. h 2 o ( g ). A chemical engineering view of a fullscale carbon dioxide absorber. When equilibrium was reached, there was still some C(s) remaining in the container. 2, the reaction is not at. 00159 2 (aq)32 2 3 -2. org are unblocked. Calculate the equilibrium constant for the reaction given the equation below : (4 marks) 2 NH3 (g)  N2 (g) + 3 H2 (g) 3. 50 moles of N 2 gas is mixed with 0. CH40S Chemical Equilibrium Unit Review Part A: Multiple Choice 1. 0 M and the concentration of O2 is 9. The oceans are a major sink for atmospheric carbon dioxide. For the reaction given below at 700°C, Kc = 0. 8 KJ/mol -25. A small equilibrium constant means the opposite, that the concentrations of reactants at equilibrium will be large in comparison to the concentrations of products. Carbon monoxide (CO) reacts with haemoglobin in the same way as oxygen: Hb(aq) + CO(aq) ⇋ HbCO(aq) OR Hb 4 (aq) + 4CO(aq) ⇋ Hb 4 (CO) 4 (aq). 7 × 10-2 M, and CO2 was measured to be 1. 2CO2 (g) 2CO (g) + O2 (g) DHe = -514 kJ. 55% CO by mass. 400 mole of bromine was placed into a rigid I. For a chemical equilibrium, the equilibrium constant is defined as the ratio between the product of the equilibrium concentrations of the products and the product of the equilibrium concentrations of the reactants, all raised to the power of their respective stoichiometric coefficients. 35 mol of CO and 0. that for the reverse reaction. 00-L reaction vessel. 0908 moles of H 2, 0. Hence, the majority of the carbon dioxide is not converted into carbonic acid. Due to the inability of traditional equilibrium methods to measure these values, previous estimates have relied upon kinetic measurements to provide equilibrium constants. Ebbing, Darrell D. 0 x 10-2 M [H2] = 3. Carbon monoxide reaches equilibrium with water vapour as they react to form hydrogen gas and carbon dioxide gas. The fourth O2 equilibrium binding constant, K4, measured by kinetic techniques, could be used to ana- lyze equilibrium curves for either native or cross- linked hemoglobin. 20 at 600°C. Answer the following questions. 4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). The equilibrium constant for the reaction CO(g)+H2O(g)= CO2 (g)and H2(g) is 5 How many moles of CO2 must be added to 1 litre container already containing 3 moles each of CO and H2O to make 2 M equilibrium concentration of CO - Chemistry - Chemical Kinetics. This can occur if some of the H 2 is consumed by reacting with I 2 to form more HI; in other words, a net reaction occurs in the reverse direction. ) CO (g) + 1/2 O2 (g) CO. C(graphite) + O2-->CO2 3. 000355 Atmosphere. Question 7. Definition of equilibrium constant Kp for gas phase reactions, and how to calculate Kp from Kc. It would not change because the amount of solid present at equilibrium is not important as long as there is some solid present. In the reaction of water and carbon monoxide to produce hydrogen molecules and carbon dioxide (H 2 O + CO ⇋ H 2 + CO 2 ). The CO 2 (aq) concentration is a function of the Henry's Law solubility and the partial pressure of CO 2 (g) in the air above the water. Calculate the equilibrium constant (KC) of the reaction at this temperature. 3 M), CO2 in liquid is practically zero and so is partial CO2 gas pressure at equilibrium. 14 M NO2, 0. 0 M and the concentration of O2 is 9. The Le Châtelier principle states that the net reaction will be in a direction that tends to reduce the effect of the added H 2. 5, calculate Kc for Reaction 2 CO2(g)␣CO(g) + 1/2O2(g) how do i calculate kc?. 0908 moles of H 2, 0. Stress Equilibrium Shift [N2] [O2] [NO] Keq. Write the expression for K for the reaction below. ) C(s) + O2(g) <----->CO2(g) Ka. CHEMISTRY 115 EXAM I(A) 1. Problem: 0. 0 M, [NH3]eq = 0. May 04,2020 - The equilibrium constant for the reaction co+H2O=co2+H2 at a certain temperature is 2. Equilibrium Constant • If the reaction involves a pure solid or pure liquid, these species do not appear in the equilibrium constant expression: Example: CH 4(g) + H 2O(l) CO(g) + 3 H 2(g) KC = [CO(g)] [H2(g)] 3 [CH4 (g)] Note that H 2O(l) does not appear in the denominator. Thus efficiency of CO2 removal from gas depends only on kinetics (contact surface and time) in this case. The equilibrium constant K c equals 3. If an equilibrium reaction is reversed, the equilibrium constant is inverted. Note that the buffer effect does not mean that the pH of the ocean remains constant when CO2 increases; it means only that changes in pH are dampened. 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0. H2 (g) + I2 (g) ↔ 2 HI (g). Determine the concentration of all species at equilibrium. 0355% of the atmosphere (on the average) and has the Henry's Law constant K CO 2 =2 x. 35 mol of CO and 0. Balance Chemical Equations with this Calculator and view a list of previously balanced equations beginning with C. The backward rates are derived from equilibrium constants of reaction and the forward rates as shown in (7) : kbi = kfi Ki (7) In addition, the equilibrium constant of the reaction 2 can be written with that of reac-tion 1, see (8). If an equilibrium system is subjected to a change in conditions that affects these reaction rates differently (a stress), then the rates are no longer equal and the system is not at equilibrium. chemical equilibrium: a state achieved when the rates of the forward Chemical Equilibrium -. Determine the value of the equilibrium constant, Kgoal, for the reaction N2(g)+O2(g)+H2(g)⇌12N2H4(g)+NO2(g), Kgoal=? by making use of the following information: 1. Next in abundance are molecular oxygen (O2) with CO2 = 0. Calculate the equilibrium constant (KC) of the reaction at this temperature. Consider the reaction 2 CO2 ⇔ 2 CO + O2 obtained after heating 1 kmol CO2 to 3000 K. CH4(g) + 2 O2(g) <-> CO2(g) + 2 H2O(g) 3. What is the equilibrium concentration of CO? An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. We will learn more about this later in our combustion studies. 35 mol of CO and 0. Ethane and steam are fed to a steam cracker at a total pressure of 1 atm and at 1000K at a ratio of 4 mol H2O to 1 mol ethane. (c) Derive and use the equation, Kp = Kc (RT)n. changing temperature D. The general form of the balanced equation is: HA(aq) ⇌ H+(aq)+A−(aq) HA ( aq) ⇌ H + ( aq) + A − ( aq) HA is a generic acid that dissociates by splitting into A −, known as the conjugate base of the acid, and a hydrogen. 1%) of CO 2 (aq) as H 2 CO 3. At 100°C the equilibrium constant for the reaction COCl 2 (g) CO(g) + Cl 2 (g) has the value of K c = 2. The equilibrium constant K c equals 3. 2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g), K1 = 5. 1) Gas dissolution. A given reaction has one equilibrium constant at a given temperature, but it has an infinite number of sets of concentrations, called the equilibrium positions. 8 × 10-11 atm, P (O2)eq = 1. Predict the sign for the change in entropy, (S, for the reaction. equilibrium is a state in which. Zn / 002 - Zno / 00. The reaction CO (g) + H 2O(g) ↔ CO 2(g) + H 2(g) is used to increase the ratio of hydrogen in synthesis gas (mixtures of CO and H 2). b) increase the partial pressure of CO (g) at equilibrium. The resultant fitted values of the Adair constants, al, a2, and a3, were similar to those obtained when K4 was allowed to vary, and the fits. , different ion concentrations, pH and/or alkalinity) with different levels of CO2 , N2 and/or O2 in the system. aA(g) + bB(g) ⇄ cC(g) + dD(g) the pressure-based equilibrium constant, K P, is defined as follows: where P A is the partial pressure of substance A at equilibrium in atmospheres, and so. 35 mol of CO and 0. SbCl5(g) m SbCl3(g) + Cl2(g) b. 72 H2 in a 1 liter flask at 600k, what will be the pressure of H2 present when this mixture has attained equilibrium?. Having equilibrium data for sodium bicarbonate could be of significant interest due to its practicality as a candidate sorbent used in the growing industry of CO 2 capture. 3H2(g) + N2(g) ( 2NH3(g) 2H2O(g) ( 2H2(g) + O2(g) The units for Keq. If we raise the temperature we add more heat to this equilibrium reaction. The dissolved gas and the undissolved gas are in equilibrium. Outline • Henry's Law • Oxygen in Equilibrium • Carbon Dioxide in Equilibrium • Homework. This can occur if some of the H 2 is consumed by reacting with I 2 to form more HI; in other words, a net reaction occurs in the reverse direction. (Similar to Rule 3; let c=the number you are dividing by. 0 M, calculate the concentration of CO. ) 2 S (s) + 3 O2 (g)CO2 (g) Kb K =_________ 2. 3M Notice the 3 sd’s in all your data. Introduction. ICE Table In the following chemical system, a 0. Removing $\ce{CO2}$ produce that $\ce{CO}$ react with $\ce{O2}$ to produce more $\ce{CO2}$. The reaction continues until a balance is established between these two processes and an equilibrium condition is reached. P4O10(s) ⇌ P4(s) + 5 O2(g) A) 20. The equilibrium constant for the formation of CO2 by the reaction 2CO (g) + O2 (g) ↔ 2 CO2 (g) is 1. 2 "The Equilibrium Constant" that the equilibrium constant for the decomposition of CaCO 3 (s) to CaO(s) and CO 2 (g) is K = [CO 2]. At a constant temperature the ratio of : CO 2 dissolved in water / CO 2 in the air is constant at a constant temperature - the so-called equilibrium constant. chemical equilibrium: a state achieved when the rates of the forward Chemical Equilibrium -. Concentrations or gas pressures of reactants and products at equilibrium can be calculated from the initial concentrations or gas pressures of reactants and products and equilibrium constants. The percent of carbon dioxide gas present in retort smelting as taken from several sources is Iwhile that present in electric furnace smelting is very likely to he more than I %, Study of the Equilibrium of the Reaction. 8 torr) ÷ (760 torr / atm) = 0. Stoichiometry. 0L flask contains: 0. In your textbook, read about calculating equilibrium concentrations. CH40S Chemical Equilibrium Unit Review Part A: Multiple Choice 1. Where, ΔG ° is the standard free change of a reaction, value of ΔG ° is -35000 (calculated in part(a)) R = gas constant, value of R is 8. This equation says that CO 2 can be converted to a mixture of CO and O2, while CO plus O2 can convert to CO 2. low temperature carbon dioxide does not react with carbon to produce carbon monoxide. May 04,2020 - The equilibrium constant for the reaction co+H2O=co2+H2 at a certain temperature is 2. 1M each of CO and H2O at 800K. 9), including one proportionality. This can occur if some of the H 2 is consumed by reacting with I 2 to form more HI; in other words, a net reaction occurs in the reverse direction. In order to balance C + O2 = CO you'll need to watch out for two things. The mixture of gases that results is an important industrial fuel called water gas (a) At 800 ºC, the equilibrium constant for this reaction is Kc = 0. At constant temperature, for Le Chatêlier purposes, Adding $\ce{CO}$ produces that it react with $\ce{O2}$ to produce more $\ce{CO2}$ to counteract the effect of the applied change and a new equilibrium is established. The equilibrium expression is the Henry's Law equation (@ 25 °C). CHEMICAL EQUILIBRIUM. equilibrium constant tells you that at equilibrium the concentrations of products will be much larger than the concentrations of reactants. Previously, the products of combustion were determined assuming that the reaction temperature did not reach greater than 1000 K. Calculate the equilibrium constant, Kc, for this. 003 5 atm of chlorine at 600°C. Use data from Appendix IIB to calculate the equilibrium constants at 25°C for each reaction. Outline • Henry's Law • Oxygen in Equilibrium • Carbon Dioxide in Equilibrium • Homework. Chemical Equilibrium. The equilibrium constant for the reaction is A) –4. 00 L container and allowed to come to equilibrium. 000 L vessel. 19 mol of CO remaining. the carbon dioxide gas dissolved in it fizzes out rapidly. At equilibrium, the pressure of CO = 2. An equilibrium mixture at 500 K has the following concentrations: [N2] = 3. The equilibrium constant depends on the initial concentrations. What are the equilibrium partial pressures of CO and CO2 at 1050 K if the initial partial pressures are: p CO= 1. Calculate the equilibrium partial pressures of CO2, H2 and CO. We adopted a larger uncertainty. 5 O2 X 1 CO X1 CO2 = 1 K1 (8) Using equations (6, 7 and 8), it is now possible to derive a simple. Did the equilibrium shift favour the formation of reactants or products? A catalyst was added to the system at constant volume and a new equilibrium was established. [CO] increases and [CO2] decreases D. Carbon (graphite), carbon dioxide, and carbon monoxide form an equilibrium mixture, as represented by the equation. But the equilibrium constant is too small for you to see any measurable change in pH of the water. c) Calculate Kp for the reaction. SO2 (g) + 1/2 O2 (g) SO2 (g)Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below:a. It would not change because the amount of solid present at equilibrium is not important as long as there is some solid present. Calculating an Equilibrium Constant from Equilibrium Concentrations.

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