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Question 7. For the Haber process described by the following reaction N2(g) + + 3 H₂(g) 3 2 NH3(g) The equilibrium constants as function of temperature are: Temperature (°C) Ke 95 227 300 327 427 527 Determine the temperature at which the reaction become spontaneous a. 754 °C b. 641 °C c. 368 °C d. 638 °C 12 4 0.1 0.05

Question 7. For the Haber process described by the following reaction N2(g) + + 3 H₂(g) 3 2 NH3(g) The equilibrium constants as function of temperature are: Temperature (°C) Ke 95 227 300 327 427 527 Determine the temperature at which the reaction become spontaneous a. 754 °C b. 641 °C c. 368 °C d. 638 °C 12 4 0.1 0.05

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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**Question 7.** For the Haber process described by the following reaction: \[ \text{N}_2(g) + 3 \text{H}_2(g) \rightleftharpoons 2 \text{NH}_3(g) \] The equilibrium constants as a function of temperature are: | Temperature (°C) | \( K_c \) | |------------------|-----------| | 227 | 95 | | 300 | 12 | | 327 | 4 | | 427 | 0.1 | | 527 | 0.05 | Determine the temperature at which the reaction becomes spontaneous. a. 754 °C b. 641 °C c. 368 °C d. 638 °C e. 836 °C **Explanation:** This question explores the relationship between temperature and equilibrium constant (\( K_c \)) for the Haber process, which synthesizes ammonia from nitrogen and hydrogen. The equilibrium constants decrease as temperature increases, which is typical for exothermic reactions. The task is to determine at which temperature the reaction becomes spontaneous.
Transcribed Image Text:**Question 7.** For the Haber process described by the following reaction: \[ \text{N}_2(g) + 3 \text{H}_2(g) \rightleftharpoons 2 \text{NH}_3(g) \] The equilibrium constants as a function of temperature are: | Temperature (°C) | \( K_c \) | |------------------|-----------| | 227 | 95 | | 300 | 12 | | 327 | 4 | | 427 | 0.1 | | 527 | 0.05 | Determine the temperature at which the reaction becomes spontaneous. a. 754 °C b. 641 °C c. 368 °C d. 638 °C e. 836 °C **Explanation:** This question explores the relationship between temperature and equilibrium constant (\( K_c \)) for the Haber process, which synthesizes ammonia from nitrogen and hydrogen. The equilibrium constants decrease as temperature increases, which is typical for exothermic reactions. The task is to determine at which temperature the reaction becomes spontaneous.
**Question 7.** For the Haber process described by the following reaction: \[ \text{N}_2 (g) + 3 \text{H}_2 (g) \rightleftharpoons 2 \text{NH}_3 (g) \] The equilibrium constants as a function of temperature are: | Temperature (°C) | \( K_c \) | |-------------------|-----------| | 227 | 95 | | 300 | 12 | | 327 | 4 | | 427 | 0.1 | | 527 | 0.05 | (a) Determine \( \Delta H^\circ \) for the Haber process. Options: a. -910 kJ/mol b. -91000 kJ/mol c. -91 kJ/mol d. -90660 kJ/mol e. -90650 kJ/mol --- In this question about the Haber process, the equilibrium constants (\( K_c \)) decrease with an increase in temperature, suggesting that the reaction is exothermic. The task is to determine the standard enthalpy change (\( \Delta H^\circ \)) for the process from the given data and options.
Transcribed Image Text:**Question 7.** For the Haber process described by the following reaction: \[ \text{N}_2 (g) + 3 \text{H}_2 (g) \rightleftharpoons 2 \text{NH}_3 (g) \] The equilibrium constants as a function of temperature are: | Temperature (°C) | \( K_c \) | |-------------------|-----------| | 227 | 95 | | 300 | 12 | | 327 | 4 | | 427 | 0.1 | | 527 | 0.05 | (a) Determine \( \Delta H^\circ \) for the Haber process. Options: a. -910 kJ/mol b. -91000 kJ/mol c. -91 kJ/mol d. -90660 kJ/mol e. -90650 kJ/mol --- In this question about the Haber process, the equilibrium constants (\( K_c \)) decrease with an increase in temperature, suggesting that the reaction is exothermic. The task is to determine the standard enthalpy change (\( \Delta H^\circ \)) for the process from the given data and options.
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