6. Consider the following reversible reaction. In a 3.00 liter container, the following amounts are found in equilibrium at 400 °C: 0.0420 mole N2, 0.516 mole H2 and 0.0357 mole NH3. Evaluate Kc. N2(g) + 3H2(g) 2NH3(g) (a) 0.202 (b) 1.99 (c) 16.0 (d) 4.94 (e) 0.503
6. Consider the following reversible reaction. In a 3.00 liter container, the following amounts are found in equilibrium at 400 °C: 0.0420 mole N2, 0.516 mole H2 and 0.0357 mole NH3. Evaluate Kc. N2(g) + 3H2(g) 2NH3(g) (a) 0.202 (b) 1.99 (c) 16.0 (d) 4.94 (e) 0.503
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![### Equilibrium Constant Calculation
**Problem Statement:**
Consider the following reversible reaction in a 3.00 liter container, with the following amounts found in equilibrium at 400 °C:
- 0.0420 mole N₂
- 0.516 mole H₂
- 0.0357 mole NH₃
Evaluate the equilibrium constant \( K_c \).
**Reaction:**
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]
**Options:**
(a) 0.202
(b) 1.99
(c) 16.0
(d) 4.94
(e) 0.503
**Solution Steps:**
1. **Determine Concentrations:**
- N₂: \(\frac{0.0420 \text{ moles}}{3 \text{ L}} = 0.0140 \text{ M}\)
- H₂: \(\frac{0.516 \text{ moles}}{3 \text{ L}} = 0.172 \text{ M}\)
- NH₃: \(\frac{0.0357 \text{ moles}}{3 \text{ L}} = 0.0119 \text{ M}\)
2. **Write the Expression for \( K_c \):**
\[ K_c = \frac{[\text{NH}_3]^2}{[\text{N}_2][\text{H}_2]^3} \]
3. **Substitute Values:**
\[
K_c = \frac{(0.0119)^2}{(0.0140)(0.172)^3}
\]
4. **Calculate \( K_c \):**
Complete the calculation to solve for \( K_c \), selecting the correct answer from the options provided.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff3b22dc5-b81c-452b-a8fe-ec73685697af%2F525e4554-a1dd-4a21-85c3-ad43786ab35f%2Fgmx73ti_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Equilibrium Constant Calculation
**Problem Statement:**
Consider the following reversible reaction in a 3.00 liter container, with the following amounts found in equilibrium at 400 °C:
- 0.0420 mole N₂
- 0.516 mole H₂
- 0.0357 mole NH₃
Evaluate the equilibrium constant \( K_c \).
**Reaction:**
\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \]
**Options:**
(a) 0.202
(b) 1.99
(c) 16.0
(d) 4.94
(e) 0.503
**Solution Steps:**
1. **Determine Concentrations:**
- N₂: \(\frac{0.0420 \text{ moles}}{3 \text{ L}} = 0.0140 \text{ M}\)
- H₂: \(\frac{0.516 \text{ moles}}{3 \text{ L}} = 0.172 \text{ M}\)
- NH₃: \(\frac{0.0357 \text{ moles}}{3 \text{ L}} = 0.0119 \text{ M}\)
2. **Write the Expression for \( K_c \):**
\[ K_c = \frac{[\text{NH}_3]^2}{[\text{N}_2][\text{H}_2]^3} \]
3. **Substitute Values:**
\[
K_c = \frac{(0.0119)^2}{(0.0140)(0.172)^3}
\]
4. **Calculate \( K_c \):**
Complete the calculation to solve for \( K_c \), selecting the correct answer from the options provided.
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