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2. A vessel at 415 K initial contains 0.40 atm N2, 0.30 atm H2, and 0.50 atm NH3. At equilibrium, the total pressure is 1.40 atm. Calculate K, and K̟ for the reaction at 415 K. N2(9) + 3H2(g) = 2NH3(g)

2. A vessel at 415 K initial contains 0.40 atm N2, 0.30 atm H2, and 0.50 atm NH3. At equilibrium, the total pressure is 1.40 atm. Calculate K, and K̟ for the reaction at 415 K. N2(9) + 3H2(g) = 2NH3(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
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**Problem 2: Equilibrium Calculations for Ammonia Synthesis** A vessel at 415 K initially contains 0.40 atm of \( \text{N}_2 \), 0.30 atm of \( \text{H}_2 \), and 0.50 atm of \( \text{NH}_3 \). At equilibrium, the total pressure is 1.40 atm. Calculate \( K_p \) and \( K_c \) for the reaction at 415 K. **Chemical Reaction:** \[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \] **Explanation:** - **Nomenclature:** - \( \text{N}_2(g) \): Nitrogen gas - \( \text{H}_2(g) \): Hydrogen gas - \( \text{NH}_3(g) \): Ammonia gas - **Objective:** - Calculate the equilibrium constants \( K_p \) (based on partial pressures) and \( K_c \) (based on concentrations) at 415 K. - **Initial Conditions:** - Initial partial pressures: - \( \text{N}_2 \): 0.40 atm - \( \text{H}_2 \): 0.30 atm - \( \text{NH}_3 \): 0.50 atm - **Equilibrium Condition:** - Total pressure at equilibrium: 1.40 atm **Steps for Calculation:** 1. Determine the change in pressure for each gas. 2. Use the equilibrium expression to find the equilibrium constants \( K_p \) and \( K_c \). 3. Apply the ideal gas law if needed to convert between \( K_p \) and \( K_c \). This calculation involves understanding the relationship between the different components of the reaction at equilibrium and how they relate to overall pressure and concentration changes.
Transcribed Image Text:**Problem 2: Equilibrium Calculations for Ammonia Synthesis** A vessel at 415 K initially contains 0.40 atm of \( \text{N}_2 \), 0.30 atm of \( \text{H}_2 \), and 0.50 atm of \( \text{NH}_3 \). At equilibrium, the total pressure is 1.40 atm. Calculate \( K_p \) and \( K_c \) for the reaction at 415 K. **Chemical Reaction:** \[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \] **Explanation:** - **Nomenclature:** - \( \text{N}_2(g) \): Nitrogen gas - \( \text{H}_2(g) \): Hydrogen gas - \( \text{NH}_3(g) \): Ammonia gas - **Objective:** - Calculate the equilibrium constants \( K_p \) (based on partial pressures) and \( K_c \) (based on concentrations) at 415 K. - **Initial Conditions:** - Initial partial pressures: - \( \text{N}_2 \): 0.40 atm - \( \text{H}_2 \): 0.30 atm - \( \text{NH}_3 \): 0.50 atm - **Equilibrium Condition:** - Total pressure at equilibrium: 1.40 atm **Steps for Calculation:** 1. Determine the change in pressure for each gas. 2. Use the equilibrium expression to find the equilibrium constants \( K_p \) and \( K_c \). 3. Apply the ideal gas law if needed to convert between \( K_p \) and \( K_c \). This calculation involves understanding the relationship between the different components of the reaction at equilibrium and how they relate to overall pressure and concentration changes.
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