Equilibrium Question 671
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 $
BETA
