Question:medium
For a given reversible reaction at \(300\,K\):
\[ 2\text{N}_2\text{O}_5(g) \rightleftharpoons 4\text{NO}_2(g) + \text{O}_2(g) \]
If \( \text{N}_2\text{O}_5 \) is 50% dissociated at 5 bar and 300 K at equilibrium, then find \( \Delta G^\circ \) for the reaction?
[Given: \( \log 2 = 0.3,\ \log 7 = 0.84 \)]
For a given reversible reaction at \(300\,K\):
\[ 2\text{N}_2\text{O}_5(g) \rightleftharpoons 4\text{NO}_2(g) + \text{O}_2(g) \]
If \( \text{N}_2\text{O}_5 \) is 50% dissociated at 5 bar and 300 K at equilibrium, then find \( \Delta G^\circ \) for the reaction?
[Given: \( \log 2 = 0.3,\ \log 7 = 0.84 \)]
Updated On: Apr 5, 2026
- \(-4\,\text{kJ}\)
- \(-8\,\text{kJ}\)
- \(-6\,\text{kJ}\)
- \(-10\,\text{kJ}\)
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The Correct Option is B
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