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6) Starting with equal moles of reactants, which of the following equilibrium systems most favors the products? A. SO; (g) + NO2 (g) € → SO; (g)+ NO (g) B. CO (g) + H2O (g) +→CO2 (g) + H2 (g) C. H2 (g) + I2 (g) € → 2HI D. N2 (g) + O2 (g) E → 2NO (g) K = 3.4 К-31.4 K = 10.0 K= 1.0 x 10-31 а) А b. В с. С d. D

6) Starting with equal moles of reactants, which of the following equilibrium systems most favors the products? A. SO; (g) + NO2 (g) € → SO; (g)+ NO (g) B. CO (g) + H2O (g) +→CO2 (g) + H2 (g) C. H2 (g) + I2 (g) € → 2HI D. N2 (g) + O2 (g) E → 2NO (g) K = 3.4 К-31.4 K = 10.0 K= 1.0 x 10-31 а) А b. В с. С d. D

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 6 Starting with equal moles of reactants, which of the following equilibrium systems most favors the products? #### Options: A. \( \text{SO}_2 (g) + \text{NO}_2 (g) \rightleftharpoons \text{SO}_3 (g) + \text{NO} (g) \) \( K = 3.4 \) B. \( \text{CO} (g) + \text{H}_2\text{O} (g) \rightleftharpoons \text{CO}_2 (g) + \text{H}_2 (g) \) \( K = 31.4 \) C. \( \text{H}_2 (g) + \text{I}_2 (g) \rightleftharpoons 2\text{HI} (g) \) \( K = 10.0 \) D. \( \text{N}_2 (g) + \text{O}_2 (g) \rightleftharpoons 2\text{NO} (g) \) \( K = 1.0 \times 10^{-31} \) ### Answer Choices: - a) A - b) B - c) C - d) D ### Explanation The equilibrium constant \( K \) indicates the extent to which a reaction favors products under a given set of conditions. A larger \( K \) value means that, at equilibrium, the concentration of products is greater in comparison to the reactants. Thus, in this question, system B with \( K = 31.4 \) most favors the products.
Transcribed Image Text:### Question 6 Starting with equal moles of reactants, which of the following equilibrium systems most favors the products? #### Options: A. \( \text{SO}_2 (g) + \text{NO}_2 (g) \rightleftharpoons \text{SO}_3 (g) + \text{NO} (g) \) \( K = 3.4 \) B. \( \text{CO} (g) + \text{H}_2\text{O} (g) \rightleftharpoons \text{CO}_2 (g) + \text{H}_2 (g) \) \( K = 31.4 \) C. \( \text{H}_2 (g) + \text{I}_2 (g) \rightleftharpoons 2\text{HI} (g) \) \( K = 10.0 \) D. \( \text{N}_2 (g) + \text{O}_2 (g) \rightleftharpoons 2\text{NO} (g) \) \( K = 1.0 \times 10^{-31} \) ### Answer Choices: - a) A - b) B - c) C - d) D ### Explanation The equilibrium constant \( K \) indicates the extent to which a reaction favors products under a given set of conditions. A larger \( K \) value means that, at equilibrium, the concentration of products is greater in comparison to the reactants. Thus, in this question, system B with \( K = 31.4 \) most favors the products.
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