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The differential rate law for the reactin
`H_2(g)+I_2(g)⇌ 2HI(g)` is
A. |
`(-d[I_2])/dt=(-d[H_2])/dt=(d[HI])/dt` |
B. |
`(d[H_2])/dt=(d[I_2])/dt=(d[HI])/dt` |
C. |
`1/2(d[H_2])/dt=1/2(d[I_2])/dt=(-d[HI_2])/dt` |
D. |
`(-2d[H_2])/dt=(-2d[I_2])/dt=(d[HI])/dt` |
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