Question 27 At 25 C, K = 0.0900 for the reaction A(g) + B(g) 2 C(g). Calculate the concentration of C(g) at equilibrium if the s 0.0261M 0.548 M 1.10 M 2.86 M O 1.17 M Moving to another question will save this response. MacBook
Question 27 At 25 C, K = 0.0900 for the reaction A(g) + B(g) 2 C(g). Calculate the concentration of C(g) at equilibrium if the s 0.0261M 0.548 M 1.10 M 2.86 M O 1.17 M Moving to another question will save this response. MacBook
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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If the starting mixture has 3.6 mol A(g), 3.6 mol B(g) and 1.2 mol C(g) in a 2L container
![### Question 27
At 25°C, \( K = 0.0900 \) for the reaction \( \text{A(g)} + \text{B(g)} \rightleftharpoons 2 \text{C(g)} \). Calculate the concentration of \( \text{C(g)} \) at equilibrium if the starting concentrations of both \( \text{A(g)} \) and \( \text{B(g)} \) are 1.00 M.
- \(\bigcirc\) 0.0261 M
- \(\bigcirc\) 0.548 M
- \(\bigcirc\) 1.10 M
- \(\bigcirc\) 2.86 M
- \(\bigcirc\) 1.17 M
\(\triangle\) Moving to another question will save this response.
Explanation:
This question involves calculating the equilibrium concentration of a product in a given chemical reaction using the equilibrium constant \( K \).
#### Step-by-step approach:
1. **Write the equilibrium expression:**
For the reaction \( \text{A(g)} + \text{B(g)} \rightleftharpoons 2 \text{C(g)} \), the equilibrium constant, K, is given by
\[
K = \frac{[\text{C(g)}]^2}{[\text{A(g)}][\text{B(g)}]}.
\]
2. **Set up the ICE table (Initial, Change, Equilibrium):**
| | A(g) | B(g) | C(g) |
|-------|--------|--------|-------|
| Initial (M) | 1.00 | 1.00 | 0 |
| Change (M) | -x | -x | +2x |
| Equilibrium | 1.00-x| 1.00-x| 2x |
3. **Substitute the equilibrium concentrations into the equilibrium expression:**
\[
K = \frac{(2x)^2}{(1.00-x)(1.00-x)} = 0.0900.
\]
4. **Solve for x:** This involves solving a quadratic equation, which yields the equilibrium concentrations.
5. **Calculate the equilibrium concentration of \( \text{C(g)} \).**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F08c67838-b49a-475f-ad93-59e7305e5b28%2F6b1c77c7-38ce-431d-9a05-3c7e8b913b85%2F53h5bn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Question 27
At 25°C, \( K = 0.0900 \) for the reaction \( \text{A(g)} + \text{B(g)} \rightleftharpoons 2 \text{C(g)} \). Calculate the concentration of \( \text{C(g)} \) at equilibrium if the starting concentrations of both \( \text{A(g)} \) and \( \text{B(g)} \) are 1.00 M.
- \(\bigcirc\) 0.0261 M
- \(\bigcirc\) 0.548 M
- \(\bigcirc\) 1.10 M
- \(\bigcirc\) 2.86 M
- \(\bigcirc\) 1.17 M
\(\triangle\) Moving to another question will save this response.
Explanation:
This question involves calculating the equilibrium concentration of a product in a given chemical reaction using the equilibrium constant \( K \).
#### Step-by-step approach:
1. **Write the equilibrium expression:**
For the reaction \( \text{A(g)} + \text{B(g)} \rightleftharpoons 2 \text{C(g)} \), the equilibrium constant, K, is given by
\[
K = \frac{[\text{C(g)}]^2}{[\text{A(g)}][\text{B(g)}]}.
\]
2. **Set up the ICE table (Initial, Change, Equilibrium):**
| | A(g) | B(g) | C(g) |
|-------|--------|--------|-------|
| Initial (M) | 1.00 | 1.00 | 0 |
| Change (M) | -x | -x | +2x |
| Equilibrium | 1.00-x| 1.00-x| 2x |
3. **Substitute the equilibrium concentrations into the equilibrium expression:**
\[
K = \frac{(2x)^2}{(1.00-x)(1.00-x)} = 0.0900.
\]
4. **Solve for x:** This involves solving a quadratic equation, which yields the equilibrium concentrations.
5. **Calculate the equilibrium concentration of \( \text{C(g)} \).**
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