mixture of 0.856 mol of NO, 0.656 mol of H₂, and 1.16 mol of H₂O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: NO(g) + 2H₂(g) = N2(g) + 2H₂O(g) At equilibrium [NO] = 0.248 M. Part B Calculate the equilibrium concentration of N₂. Express the molarity to three decimal places. VE ΑΣΦ Submit Part C Calculate the equilibrium concentration of H₂O. Express the molarity to three decimal places. [5] ΑΣΦ Submit Request Answer Part D Request Answer Calculate Ke Express your answer to two significant figures. ? ? M M
mixture of 0.856 mol of NO, 0.656 mol of H₂, and 1.16 mol of H₂O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: NO(g) + 2H₂(g) = N2(g) + 2H₂O(g) At equilibrium [NO] = 0.248 M. Part B Calculate the equilibrium concentration of N₂. Express the molarity to three decimal places. VE ΑΣΦ Submit Part C Calculate the equilibrium concentration of H₂O. Express the molarity to three decimal places. [5] ΑΣΦ Submit Request Answer Part D Request Answer Calculate Ke Express your answer to two significant figures. ? ? M M
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help with c and d
![### Equilibrium Calculation Exercise
**Scenario:**
A mixture of 0.856 moles of NO, 0.656 moles of H₂, and 1.16 moles of H₂O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established:
\[ 2\text{NO}(g) + 2\text{H}_2(g) \rightleftharpoons \text{N}_2(g) + 2\text{H}_2\text{O}(g) \]
At equilibrium, \([\text{NO}] = 0.248\ M.\)
---
**Tasks:**
- **Part B:** (Note: This section is crossed out and not to be addressed.)
- Calculate the equilibrium concentration of \(\text{N}_2\).
- Express the molarity to three decimal places.
---
- **Part C:**
- **Objective:** Calculate the equilibrium concentration of \(\text{H}_2\text{O}\).
- **Instruction:** Express the molarity to three decimal places.
- **Input Box:** An input field is provided for entering your response.
- **Submit Button:** Click to submit your answer.
---
- **Part D:**
- **Objective:** Calculate the equilibrium constant, \(K_c\).
- **Instruction:** Express your answer to two significant figures.
- **Input Box:** An input field is provided for entering your response.
- **Submit Button:** Click to submit your answer.
---
**Note:** Use stoichiometry and equilibrium principles to calculate these values.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1205cd08-0e41-4ad8-bd1c-6b97372ee2c1%2F0fbd73b9-b767-4c3f-89c5-c090b44187ba%2Fjk0y02f_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Equilibrium Calculation Exercise
**Scenario:**
A mixture of 0.856 moles of NO, 0.656 moles of H₂, and 1.16 moles of H₂O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established:
\[ 2\text{NO}(g) + 2\text{H}_2(g) \rightleftharpoons \text{N}_2(g) + 2\text{H}_2\text{O}(g) \]
At equilibrium, \([\text{NO}] = 0.248\ M.\)
---
**Tasks:**
- **Part B:** (Note: This section is crossed out and not to be addressed.)
- Calculate the equilibrium concentration of \(\text{N}_2\).
- Express the molarity to three decimal places.
---
- **Part C:**
- **Objective:** Calculate the equilibrium concentration of \(\text{H}_2\text{O}\).
- **Instruction:** Express the molarity to three decimal places.
- **Input Box:** An input field is provided for entering your response.
- **Submit Button:** Click to submit your answer.
---
- **Part D:**
- **Objective:** Calculate the equilibrium constant, \(K_c\).
- **Instruction:** Express your answer to two significant figures.
- **Input Box:** An input field is provided for entering your response.
- **Submit Button:** Click to submit your answer.
---
**Note:** Use stoichiometry and equilibrium principles to calculate these values.
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