General Chemistry: Principles and Modern Applications (10th Edition)

Published by Pearson Prentice Hal
ISBN 10: 0132064529
ISBN 13: 978-0-13206-452-1

Chapter 15 - Priciples of Chemical Equilibrium - Exercises - Equilibrium Relationshipos - Page 689: 27


(a) $\Delta n = 0$, so the volume does not affect the equilibrium constant. (b) $K_c = K_p = 0.659$

Work Step by Step

(a) There are 2 moles of gaseous reactants and 2 moles of gaseous products. $\Delta n = 0$, therefore, the change in volume will not affect the equilibrium. Mathematically: $$K_c = \frac{[CO][H_2O]}{[CO_2][H_2]}$$ Since molarity is number of moles divided by volume: $$K_c = \frac{\frac{n_{CO}}{V}{}\frac{n_{H_2O}}{V}}{\frac{n_{CO_2}}{V}\frac{n_{H_2}}{V}}$$ Simplifying: $$K_c = \frac{{n_{CO}}{}{}{n_{H_2O}}{}}{{n_{CO_2}}{}{n_{H_2}}{}}$$ The Volume do not appear on the equilibrium constant expression. (b) Substitute: $$K_c = \frac{(0.224)(0.224)}{(0.276)(0.276)} = 0.659$$ $$K_p = K_c(RT)^{\Delta n} = K_c(RT)^0 = K_c(1) = K_c = 0.659$$
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