question_answer

    For the reaction:\[{{H}_{2}}+{{I}_{2}}\xrightarrow[{}]{{}}2HI,\]the differential rate law is:

A)  \[-\frac{d[{{H}_{2}}]}{dt}=-\frac{d[{{I}_{2}}]}{dt}=2\frac{d[HI[}{dt}\]

B)  \[-2\frac{d[{{H}_{2}}]}{dt}=-2\frac{d[{{I}_{2}}]}{dt}=\frac{d[HI]}{dt}\]

C)  \[-\frac{d[{{H}_{2}}]}{dt}=-\frac{d[{{I}_{2}}]}{dt}=\frac{d[HI]}{dt}\]

D)  \[-\frac{d[{{H}_{2}}]}{2dt}=-\frac{d[{{I}_{2}}]}{2dt}=\frac{d[HI]}{dt}\]