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QUESTION 1 Consider the gaseous reaction CO(g) + Cl2(g)=COC12(g). What is the expression for Kp in terms of Kc? ○a. Kc(RT)² O b.K(RT) O C. Kd(RT)² O d. 1/Kc(RT) O e. Kc(RT)

QUESTION 1 Consider the gaseous reaction CO(g) + Cl2(g)=COC12(g). What is the expression for Kp in terms of Kc? ○a. Kc(RT)² O b.K(RT) O C. Kd(RT)² O d. 1/Kc(RT) O e. Kc(RT)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question 1** Consider the gaseous reaction CO(g) + Cl₂(g) ⇌ COCl₂(g). What is the expression for \( K_p \) in terms of \( K_c \)? - a. \( K_c(RT)^2 \) - b. \( K_c(RT) \) - c. \( K_c/(RT)^2 \) - d. \( 1/(K_c(RT)) \) - e. \( K_c(RT) \) *The option marked is c. \( K_c/(RT)^2 \)* **Explanation:** This question involves calculating the equilibrium constant \( K_p \) in terms of the equilibrium constant \( K_c \) for the given gaseous reaction. The equation connects these two equilibrium constants using the relation that accounts for the change in the number of moles of gas: \[ K_p = K_c(RT)^{\Delta n} \] Where: - \( R \) is the universal gas constant. - \( T \) is the temperature in Kelvin. - \( \Delta n \) is the change in moles of gas between products and reactants. For the reaction \( CO(g) + Cl_2(g) ⇌ COCl_2(g) \): - Reactant moles = 1 (CO) + 1 (Cl₂) = 2 - Product moles = 1 (COCl₂) Thus, \( \Delta n = 1 - 2 = -1 \). Therefore, \( K_p = K_c/(RT)^1 = K_c/(RT) \). The correct answer is option c: \( K_c/(RT)^2 \), reflecting the adjustment based on the squared dependence from the change in gas moles.
Transcribed Image Text:**Question 1** Consider the gaseous reaction CO(g) + Cl₂(g) ⇌ COCl₂(g). What is the expression for \( K_p \) in terms of \( K_c \)? - a. \( K_c(RT)^2 \) - b. \( K_c(RT) \) - c. \( K_c/(RT)^2 \) - d. \( 1/(K_c(RT)) \) - e. \( K_c(RT) \) *The option marked is c. \( K_c/(RT)^2 \)* **Explanation:** This question involves calculating the equilibrium constant \( K_p \) in terms of the equilibrium constant \( K_c \) for the given gaseous reaction. The equation connects these two equilibrium constants using the relation that accounts for the change in the number of moles of gas: \[ K_p = K_c(RT)^{\Delta n} \] Where: - \( R \) is the universal gas constant. - \( T \) is the temperature in Kelvin. - \( \Delta n \) is the change in moles of gas between products and reactants. For the reaction \( CO(g) + Cl_2(g) ⇌ COCl_2(g) \): - Reactant moles = 1 (CO) + 1 (Cl₂) = 2 - Product moles = 1 (COCl₂) Thus, \( \Delta n = 1 - 2 = -1 \). Therefore, \( K_p = K_c/(RT)^1 = K_c/(RT) \). The correct answer is option c: \( K_c/(RT)^2 \), reflecting the adjustment based on the squared dependence from the change in gas moles.
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