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At a certain temperature, the equilibrium constant K for the following reaction is 1.3: NO₂(g) + CO(g) →NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 45. L reaction vessel is filled with 1.1 mol of NO and 1.1 mol of CO2. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. NO(g) + CO2(9) NO ₂(g) + CO (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(9)+2CO(g) 2NO(g)+2CO₂(g) O There will be very little NO₂ and CO. O There will be very little NO and CO2₂. O Neither of the above is true. K = K = 0

At a certain temperature, the equilibrium constant K for the following reaction is 1.3: NO₂(g) + CO(g) →NO(g) + CO₂(g) Use this information to complete the following table. Suppose a 45. L reaction vessel is filled with 1.1 mol of NO and 1.1 mol of CO2. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. NO(g) + CO2(9) NO ₂(g) + CO (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. 2 NO₂(9)+2CO(g) 2NO(g)+2CO₂(g) O There will be very little NO₂ and CO. O There will be very little NO and CO2₂. O Neither of the above is true. K = K = 0

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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### 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.
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.
Expert Solution
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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