Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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### Understanding Equilibrium Constant \( K \) for Chemical Reactions At a certain temperature, the equilibrium constant \( K \) for the reaction: \[ \text{NO}_2(g) + \text{CO}(g) \rightleftharpoons \text{NO}(g) + \text{CO}_2(g) \] is given as 1.3. Use this information to complete the following exercises. #### Problem 1: Analyzing the Reaction Mixture Suppose a 45 L reaction vessel is filled with 1.1 mol of NO and 1.1 mol of CO\(_2\). What can you infer about the composition of the mixture at equilibrium? - **Options:** - There will be very little NO\(_2\) and CO. - There will be very little NO and CO\(_2\). - Neither of the above is true. #### Problem 2: Calculating Equilibrium Constants 1. **For the reaction:** \[ \text{NO}(g) + \text{CO}_2(g) \rightleftharpoons \text{NO}_2(g) + \text{CO}(g) \] - What is the equilibrium constant for this reaction? - **Round your answer to 2 significant digits.** - \( K = \square \) 2. **For the reaction:** \[ 2 \text{NO}_2(g) + 2 \text{CO}(g) \rightleftharpoons 2 \text{NO}(g) + 2 \text{CO}_2(g) \] - What is the equilibrium constant for this reaction? - **Round your answer to 2 significant digits.** - \( K = \square \) This exercise encourages students to consider the stoichiometry and equilibrium of chemical reactions, emphasizing the significance of \( K \) in predicting reaction behavior under different conditions.
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Transcribed Image Text:### Understanding Equilibrium Constant \( K \) for Chemical Reactions At a certain temperature, the equilibrium constant \( K \) for the reaction: \[ \text{NO}_2(g) + \text{CO}(g) \rightleftharpoons \text{NO}(g) + \text{CO}_2(g) \] is given as 1.3. Use this information to complete the following exercises. #### Problem 1: Analyzing the Reaction Mixture Suppose a 45 L reaction vessel is filled with 1.1 mol of NO and 1.1 mol of CO\(_2\). What can you infer about the composition of the mixture at equilibrium? - **Options:** - There will be very little NO\(_2\) and CO. - There will be very little NO and CO\(_2\). - Neither of the above is true. #### Problem 2: Calculating Equilibrium Constants 1. **For the reaction:** \[ \text{NO}(g) + \text{CO}_2(g) \rightleftharpoons \text{NO}_2(g) + \text{CO}(g) \] - What is the equilibrium constant for this reaction? - **Round your answer to 2 significant digits.** - \( K = \square \) 2. **For the reaction:** \[ 2 \text{NO}_2(g) + 2 \text{CO}(g) \rightleftharpoons 2 \text{NO}(g) + 2 \text{CO}_2(g) \] - What is the equilibrium constant for this reaction? - **Round your answer to 2 significant digits.** - \( K = \square \) This exercise encourages students to consider the stoichiometry and equilibrium of chemical reactions, emphasizing the significance of \( K \) in predicting reaction behavior under different conditions.
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Step 1: Equilibrium constant expression for the given reaction

Answer:

Given reaction:

NO subscript 2 left parenthesis straight g right parenthesis plus CO left parenthesis straight g right parenthesis rightwards harpoon over leftwards harpoon NO left parenthesis straight g right parenthesis plus CO subscript 2 left parenthesis straight g right parenthesis

equilibrium constant expression for the above reaction is:

straight K equals fraction numerator left square bracket NO right square bracket left square bracket CO subscript 2 right square bracket over denominator left square bracket NO subscript 2 right square bracket left square bracket CO right square bracket end fraction space space space space space space space space...... equation left parenthesis 1 right parenthesis

Here value of K is 1.3

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