JEE MAIN - Chemistry (2004 - No. 6)
The equilibrium constant for the reaction N2(g) + O2(g) $$\leftrightharpoons$$ 2NO(g) at temperature T is
4 $$\times$$ 10-4. The value of Kc for the reaction NO(g) $$\leftrightharpoons$$ $$1 \over 2$$N2 (g) + $$1 \over 2$$O2 (g) at the same temperature is :
2.5 $$\times$$ 102
4 $$\times$$ 10-4
50
0.02
Explanation
$${K_c} = {{{{\left[ {NO} \right]}^2}} \over {\left[ {{N_2}} \right]\left[ {{O_2}} \right]}} = 4 \times {10^{ - 4}}$$
$$K{'_c} = {{{{\left[ {{N_2}} \right]}^{1/2}}{{\left[ {{Q_2}} \right]}^{1/2}}} \over {\left[ {NO} \right]}}$$
$$ = {1 \over {\sqrt {{K_c}} }}$$
$$ = {1 \over {\sqrt {4 \times {{10}^{ - 4}}} }}$$
$$ = 50$$
$$K{'_c} = {{{{\left[ {{N_2}} \right]}^{1/2}}{{\left[ {{Q_2}} \right]}^{1/2}}} \over {\left[ {NO} \right]}}$$
$$ = {1 \over {\sqrt {{K_c}} }}$$
$$ = {1 \over {\sqrt {4 \times {{10}^{ - 4}}} }}$$
$$ = 50$$
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