For the reaction: $H_{2} + I_{2} \longrightarrow 2 HI$,the differential rate law is
- A$-\frac{d[H_{2}]}{dt} = -\frac{d[I_{2}]}{dt} = 2 \frac{d[HI]}{dt}$
- B$-\frac{d[H_{2}]}{dt} = -\frac{d[I_{2}]}{dt} = \frac{1}{2} \frac{d[HI]}{dt}$
- C$-\frac{d[H_{2}]}{dt} = -\frac{d[I_{2}]}{dt} = \frac{d[HI]}{dt}$
- D$-\frac{d[H_{2}]}{dt} = -\frac{d[I_{2}]}{dt} = \frac{1}{4} \frac{d[HI]}{dt}$
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