### Equilibrium Calculations#### Problem 2**Equilibrium Reaction:**\[ 2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g) \]**Given Equilibrium Concentrations:**- \([\text{SO}_2] = 5.6 \times 10^{-3} \, \text{M}\)- \([\text{SO}_3] = 1.6 \times 10^{-2} \, \text{M}\)- \([\text{O}_2] = 2.1 \times 10^{-3} \, \text{M}\)**Task:**Determine the equilibrium constant \( K \).#### Problem 3**Equilibrium Reaction:**\[ 2\text{H}_2\text{S}(g) + \text{CH}_4(g) \rightleftharpoons 4\text{H}_2(g) + \text{CS}_2(g) \]**Given Data:**- Equilibrium constant \( K = 4.56 \)- \([\text{H}_2\text{S}(g)] = 0.15 \, \text{M}\)- \([\text{CH}_4] = 0.56 \, \text{M}\)- \([\text{CS}_2] = 0.37 \, \text{M}\)**Task:**Determine the equilibrium concentration of \(\text{H}_2\).

Answered: [2] Consider the equilibrium: 2SO2(g) +…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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### Equilibrium Calculations

#### Problem 2
**Equilibrium Reaction:**
\[ 2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g) \]

**Given Equilibrium Concentrations:**
- \([\text{SO}_2] = 5.6 \times 10^{-3} \, \text{M}\)
- \([\text{SO}_3] = 1.6 \times 10^{-2} \, \text{M}\)
- \([\text{O}_2] = 2.1 \times 10^{-3} \, \text{M}\)

**Task:**
Determine the equilibrium constant \( K \).

#### Problem 3
**Equilibrium Reaction:**
\[ 2\text{H}_2\text{S}(g) + \text{CH}_4(g) \rightleftharpoons 4\text{H}_2(g) + \text{CS}_2(g) \]

**Given Data:**
- Equilibrium constant \( K = 4.56 \)
- \([\text{H}_2\text{S}(g)] = 0.15 \, \text{M}\)
- \([\text{CH}_4] = 0.56 \, \text{M}\)
- \([\text{CS}_2] = 0.37 \, \text{M}\)

**Task:**
Determine the equilibrium concentration of \(\text{H}_2\).

Expert Solution

Step 1: Concept of Equilibrium constant

Equilibrium constant Kc for a reaction is defined as the product of the molar concentrations of the products, each raised to the power equal to a stoichiometric coefficient divided by the product of the molar concentrations of the reactant each raised to the power equal to its stoichiometric coefficient .
& the most important convention to be kept in mind is that the active mass of a pure solid or pure liquid is considered to be constant.

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