For the reactions $NO_{(g)} + 1/2 O_{2(g)} \rightleftharpoons NO_{2(g)}$ and $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,the equilibrium constants at a given temperature are $K_1$ and $K_2$ respectively. If the value of $K_1$ is $4 \times 10^{-3}$,then the value of $K_2$ will be ....
- A$8 \times 10^{-3}$
- B$16 \times 10^{-3}$
- C$6.25 \times 10^{4}$
- D$6.25 \times 10^{6}$
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