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The Kp for the reaction A (g) reaction 2 A (g) = 4B (g)?

The Kp for the reaction A (g) reaction 2 A (g) = 4B (g)?

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:** The \( K_p \) for the reaction \( \text{A} \, (g) \rightleftharpoons 2 \, \text{B} \, (g) \) is 0.0730. What is \( K_p \) for the reaction \( 2 \, \text{A} \, (g) \rightleftharpoons 4 \, \text{B} \, (g) \)? **Answer Options:** The image includes a simple calculator interface without answer options provided directly. **Explanation:** To solve this question, consider the relation between the two reactions: 1. Original reaction: \( \text{A} \, (g) \rightleftharpoons 2 \, \text{B} \, (g) \) - \( K_p = 0.0730 \) 2. New reaction: \( 2 \, \text{A} \, (g) \rightleftharpoons 4 \, \text{B} \, (g) \) The new reaction is essentially the original reaction multiplied by 2. When a chemical equation is multiplied by a factor, the equilibrium constant is raised to the power of that factor. Thus, \( K_p \) for the new reaction is: \[ K_p = (0.0730)^2 \approx 0.005329 \] Therefore, the \( K_p \) for the reaction \( 2 \, \text{A} \, (g) \rightleftharpoons 4 \, \text{B} \, (g) \) would be approximately 0.005329. **Calculator Interface:** The calculator interface suggests basic arithmetic operations can be performed directly, though it is unclear if multiple functions or advanced calculations are enabled.
Transcribed Image Text:**Question:** The \( K_p \) for the reaction \( \text{A} \, (g) \rightleftharpoons 2 \, \text{B} \, (g) \) is 0.0730. What is \( K_p \) for the reaction \( 2 \, \text{A} \, (g) \rightleftharpoons 4 \, \text{B} \, (g) \)? **Answer Options:** The image includes a simple calculator interface without answer options provided directly. **Explanation:** To solve this question, consider the relation between the two reactions: 1. Original reaction: \( \text{A} \, (g) \rightleftharpoons 2 \, \text{B} \, (g) \) - \( K_p = 0.0730 \) 2. New reaction: \( 2 \, \text{A} \, (g) \rightleftharpoons 4 \, \text{B} \, (g) \) The new reaction is essentially the original reaction multiplied by 2. When a chemical equation is multiplied by a factor, the equilibrium constant is raised to the power of that factor. Thus, \( K_p \) for the new reaction is: \[ K_p = (0.0730)^2 \approx 0.005329 \] Therefore, the \( K_p \) for the reaction \( 2 \, \text{A} \, (g) \rightleftharpoons 4 \, \text{B} \, (g) \) would be approximately 0.005329. **Calculator Interface:** The calculator interface suggests basic arithmetic operations can be performed directly, though it is unclear if multiple functions or advanced calculations are enabled.
Expert Solution
Step 1: Equilibrium constant

The equilibrium constants accompanied by an ideal gaseous mixture are signified as Kp and Kc. When the equilibrium concentrations are described in terms of atmospheric pressure, the equilibrium constant Kp is utilized. Kp serves as an equilibrium constant accounted using the partial pressures that imply the product-reactant ratio in an equilibrium chemical reaction.

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