(Incorrect) 2 H₂S(g) + 2 H₂(g) + S₂(g) Kc = 9.3x 108 at 400°C 3.5 moles of H₂S are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of H₂ at equilibrium. 3.1 x 10-3 M (Your answer) 4.8 x 10-3 M 2.7 x 10-8 M 3.2 × 10-4 M 6.3 x 10-3 M (Correct answer)

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### Equilibrium Calculation Example

**Problem:**

Given the reaction: 

\[ 2 \text{H}_2\text{S(g)} \rightleftharpoons 2 \text{H}_2\text{(g)} + \text{S}_2\text{(g)} \]

where \( K_c = 9.3 \times 10^{-8} \) at 400°C.

3.5 moles of \(\text{H}_2\text{S}\) are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of \(\text{H}_2\) at equilibrium.

**Options:**

1. **3.1 × 10⁻³ M** (Your answer)
2. **4.8 × 10⁻³ M**
3. **2.7 × 10⁻⁸ M**
4. **3.2 × 10⁻⁴ M**
5. **6.3 × 10⁻³ M** (Correct answer)
Transcribed Image Text:### Equilibrium Calculation Example **Problem:** Given the reaction: \[ 2 \text{H}_2\text{S(g)} \rightleftharpoons 2 \text{H}_2\text{(g)} + \text{S}_2\text{(g)} \] where \( K_c = 9.3 \times 10^{-8} \) at 400°C. 3.5 moles of \(\text{H}_2\text{S}\) are placed in a 3.0 L container and the system is allowed to reach equilibrium. Calculate the concentration of \(\text{H}_2\) at equilibrium. **Options:** 1. **3.1 × 10⁻³ M** (Your answer) 2. **4.8 × 10⁻³ M** 3. **2.7 × 10⁻⁸ M** 4. **3.2 × 10⁻⁴ M** 5. **6.3 × 10⁻³ M** (Correct answer)
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