The free energy of formation of NO is 78kJmol−1 at the temperature of 1000K. What is the equilibrium constant for this reaction at 1000K? 12N2(g)+12O2(g)⇌NO(g)
A
8.4×10−5
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B
7.1×10−9
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C
4.2×10−10
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D
1.7×10−19
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Solution
The correct option is A8.4×10−5 The relation between Gibbs free energy and K is given by −ΔG∘=2.303RTlogK
simplifying and taking antilog on both sides we get, K=anti log[−ΔG∘2.303RT]Putting the values we get,[−78×10002.303×8.314×1000]=8.4×10−5