A) \[1.95\times {{10}^{-3}}\]
B) \[1.95\times {{10}^{3}}\]
C) \[7.5\times {{10}^{2}}\]
D) \[0.9\times {{10}^{6}}\]
Correct Answer: C
Solution :
\[2N{{O}_{2}}(g)\rightleftharpoons 2NO(g)+{{O}_{2}}(g)\] \[{{K}_{c}}=\frac{{{[NO]}^{2}}[{{O}_{2}}]}{{{[N{{O}_{2}}]}^{2}}}=1.8\times {{10}^{-6}}\] For reaction \[\frac{1}{2}{{O}_{2}}(g)+NO(g)\rightleftharpoons N{{O}_{2}}(g)\] \[K_{c}^{}=\frac{[N{{O}_{2}}]}{{{[{{O}_{2}}]}^{1/2}}[NO]}=\sqrt{\frac{1}{{{K}_{c}}}}\] \[=\sqrt{\frac{1}{1.8\times {{10}^{-6}}}}=\sqrt{0.56\times {{10}^{-6}}}\] \[=0.75\times {{10}^{3}}=7.5\times {{10}^{2}}\]You need to login to perform this action.
You will be redirected in
3 sec