Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 1.5 L reaction vessel contained a mixture of 5.0 x 102 M SO,, 3.5 × 10³ M O₂, and 3.0 x 10³ M SO, at 800 K. What are the values of Kc and Kp for the reaction at this temperature? [5.0 x 10] [3.0 x 10° Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [3.5 × 10% 2[5.0 x 10"] 2 SO₂(g) + O₂(g) 2 SO₂(g) = Once the expression is constructed, solve for Kc. Complete Parts 1-2 before submitting your answer. Kc = [3.0 x 10%] 2[3.5 * 10%] [3.3 * 10%] 2[3.0 * 10%] 2 [2.3 × 10% 7.9 x 10¹ [2.0 × 10% 1.3 x 10⁰ NEXT [5.0 x 10°³ 2.1 x 10 RESET [3.5 × 10³ 4.8 × 10³ >

Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 1.5 L reaction vessel contained a mixture of 5.0 x 102 M SO,, 3.5 × 10³ M O₂, and 3.0 x 10³ M SO, at 800 K. What are the values of Kc and Kp for the reaction at this temperature? [5.0 x 10] [3.0 x 10° Based on the given data, set up the expression for Kc. Each reaction participant must be represented by one tile. Do not combine terms. [3.5 × 10% 2[5.0 x 10"] 2 SO₂(g) + O₂(g) 2 SO₂(g) = Once the expression is constructed, solve for Kc. Complete Parts 1-2 before submitting your answer. Kc = [3.0 x 10%] 2[3.5 * 10%] [3.3 * 10%] 2[3.0 * 10%] 2 [2.3 × 10% 7.9 x 10¹ [2.0 × 10% 1.3 x 10⁰ NEXT [5.0 x 10°³ 2.1 x 10 RESET [3.5 × 10³ 4.8 × 10³ >

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 66QAP: Consider the equilibrium H2(g)+S(s)H2S(g)When this system is at equilibrium at 25C in a 2.00-L...

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Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When equilibrium is established, a 2.5-L reaction vessel at 125C contains 15.0 g of R, 4.3 atm of X2, and 0.98 atm of X2R. (a) Calculate K for the reaction at 125C. (b) The mass of R is doubled. What are the partial pressures of X2 and X2R when equilibrium is reestablished? (c) The partial pressure of X2 is decreased to 2.0 atm. What are the partial pressures of X2 and X2R when equilibrium is reestablished?
A mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 5.0 103 mol/L, [O2] = 1.9 103 mol/L, and [SO3] = 6.9 103 mol/L. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 SO2(g) + O2(g) 2 SO3(g) Kc = 279
Consider the equilibrium H2(g)+S(s)H2S(g)When this system is at equilibrium at 25C in a 2.00-L container, 0.120 mol of H2, 0.034 mol of H2S, and 0.4000 mol of S are present. When the temperature is increased to 35C, the partial pressure of H2 increases to 1.56 atm. (a) What is K for the reaction at 25C? (b) What is K for the reaction at 35C?
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
The reaction PCl5(g) PCl3(g) + Cl2(g) was examined at 250 C. At equilibrium, [PCl5] = 4.2 105 mol/L, [PCl3] = 1.3 102 mol/L, and [Cl2] = 3.9 103 mol/L. Calculate Kc, for the reaction.
You place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C and 10.0 atm. The reaction is N2(g)+3H2(g)2NH3(g) What is the composition of the equilibrium mixture if you obtain 0.048 mol of ammonia, NH3, from it?
Two molecules of A react to form one molecule of B, as in the reaction 2 A(g) B(g) Three experiments are done at different temperatures and equilibrium concentrations are measured. For each experiment, calculate the equilibrium constant, Kc. (a) [A] = 0.74 mol/L, [B] = 0.74 mol/L (b) [A] = 2.0 mol/L, [B] = 2.0 mol/L (c) [A] = 0.01 mol/L, [B] = 0.01 mol/L What can you conclude about this statement: If the concentrations of reactants and products are equal, then the equilibrium constant is always 1.0.
The equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?