help **Understanding Equilibrium Constants**In this section, we are considering the equilibrium constants for two chemical reactions. The equilibrium constants are given as follows:- $ K_1 = 10.0 $- $ K_2 = 1.50 \times 10^{-8} $### Reactions1. **Reaction 1:** \[ 2C(s) + O_2(aq) \leftrightarrow 2CO(aq) \] - Equilibrium constant: $ K_1 $2. **Reaction 2:** \[ 2CO_2(aq) \leftrightarrow 2CO(aq) + O_2(aq) \] - Equilibrium constant: $ K_2 $**Question:**What is the equilibrium constant for the following chemical reaction?\[ \frac{1}{2} C(s) + \frac{1}{2} O_2(aq) \leftrightarrow \frac{1}{2} CO_2(aq) \]**Answer Choices:**- $ 2.48 \times 10^4 $- $ 2.58 \times 10^4 $- $ 6.67 \times 10^8 $- $ 9.60 $- **Selected Answer:** $ 1.61 \times 10^2 $By analyzing the given data and understanding the transformations between the given reactions, the equilibrium constant for the provided reaction can be determined using the relationship between the original constants $ K_1 $ and $ K_2 $. The correct answer, as highlighted, is $ 1.61 \times 10^2 $.

Equilibrium means it is the condition at which concentration of reactant or product are equal.…

Assuming the equilibrium constants for the following two chemical reactions are 10.0 (K1) and 1.50x10-8 (K2), respectively: 2C(s) + O2(aq) <=> 2CO(aq) K1 2CO2(aq) <=> 2CO(aq) + O2(aq) K2 What is the equilibrium constant for the chemical reaction shown below? C(s) +02(aq) <=> CO2(aq) O 2.48 x 104 2.58 x 104 6.67 x 108 9.60 1.61 x 102

Assuming the equilibrium constants for the following two chemical reactions are 10.0 (K1) and 1.50x10-8 (K2), respectively: 2C(s) + O2(aq) <=> 2CO(aq) K1 2CO2(aq) <=> 2CO(aq) + O2(aq) K2 What is the equilibrium constant for the chemical reaction shown below? C(s) +02(aq) <=> CO2(aq) O 2.48 x 104 2.58 x 104 6.67 x 108 9.60 1.61 x 102

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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**Understanding Equilibrium Constants**

In this section, we are considering the equilibrium constants for two chemical reactions. The equilibrium constants are given as follows:

- $ K_1 = 10.0 $
- $ K_2 = 1.50 \times 10^{-8} $

### Reactions

1. **Reaction 1:**
\[ 2C(s) + O_2(aq) \leftrightarrow 2CO(aq) \]
- Equilibrium constant: $ K_1 $

2. **Reaction 2:**
\[ 2CO_2(aq) \leftrightarrow 2CO(aq) + O_2(aq) \]
- Equilibrium constant: $ K_2 $

**Question:**

What is the equilibrium constant for the following chemical reaction?

\[ \frac{1}{2} C(s) + \frac{1}{2} O_2(aq) \leftrightarrow \frac{1}{2} CO_2(aq) \]

**Answer Choices:**

- $ 2.48 \times 10^4 $
- $ 2.58 \times 10^4 $
- $ 6.67 \times 10^8 $
- $ 9.60 $
- **Selected Answer:** $ 1.61 \times 10^2 $

By analyzing the given data and understanding the transformations between the given reactions, the equilibrium constant for the provided reaction can be determined using the relationship between the original constants $ K_1 $ and $ K_2 $. The correct answer, as highlighted, is $ 1.61 \times 10^2 $.

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