For the reaction: $H_2 + I_2 \to 2HI$, the differential rate law is :

Question

( A ) $\begin{align*}- \frac{d[H_2]}{dt} = - \frac{d[I_2]}{dt} = \frac{d [HI]}{dt} \end{align*}$
( B ) $\begin{align*}- \frac{d[H_2]}{2dt} = - \frac{d[I_2]}{2dt} = \frac{d [HI]}{dt} \end{align*}$
( C ) $\begin{align*}- \frac{d[H_2]}{dt} = - \frac{d[I_2]}{dt} =2 \frac{d [HI]}{dt} \end{align*}$
( D ) $\begin{align*}-2 \frac{d[H_2]}{dt} = -2 \frac{d[I_2]}{dt} = \frac{d [HI]}{dt} \end{align*}$