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Question

Which one of the following oxides is most stable? The equilibrium constants are given at the same temperature:


A
2N2O5(g)2N2(g)+5O2(g);K=1.2×1034
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B
2N2O(g)2N2(g)+O2(g);K=3.5×1035
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C
2NO(g)N2(g)+O2(g);K=2.2×1030
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D
2NO2(g)N2(g)+2O2(g);K=6.71×1016
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Solution

The correct option is B $$2N{ O }_{ 2 }(g)\rightleftharpoons { N }_{ 2 }(g)+2{ O }_{ 2 }(g);K=6.71\times { 10 }^{ 16 }$$
The following oxides is most stable as it has lowest value of the equilibrium constant.
$$2N{ O }_{ 2 }(g)\rightleftharpoons { N }_{ 2 }(g)+2{ O }_{ 2 }(g);K=6.71\times { 10 }^{ 16 }$$
Low value of the equilibrium constant means that the extent of the forward reaction is small. So the decomposition of nitrogen dioxide occurs to small extent. So the oxide has high stability.

Chemistry

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