Equilibrium Question 730

Question: The equilibrium constant for the reaction; $ {N_{2(g)}}+{O_{2(g)}} \leftrightharpoons 2N{O_{(g)}} $ at temperature T is $ 4\times {10^{-4.}} $ .The value of $ K_{c} $ for the reaction. $ N{O_{(g)}} \leftrightharpoons 1/2{N_{2(g)}}+1/2{O_{2(g)}} $ at the temperature is

Options:

A) 0.02

B) 50

C) $ 4\times {10^{-4}} $

D) $ 2.5\times {10^{-2}} $

Show Answer

Answer:

Correct Answer: B

Solution:

$ N_2+O_2\rightarrow 2NO $

$ K_{C1}=\frac{{{[NO]}^{2}}}{[N_2][O_2]}=4\times {10^{-4}} $

$ NO\rightarrow 1/2N_2+1/2O_2 $

$ {K_{C_2}}=\frac{{{[N_2]}^{1/2}}{{[O_2]}^{1/2}}}{[NO]} $

$ {K_{C_2}}=\sqrt{\frac{1}{{K_{c_1}}}}=\sqrt{\frac{1}{4\times {10^{-4}}}}=50 $



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