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Chemistry
For the reaction: H2+I2 xrightarrow[]2HI, the differential rate law is:
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Q. For the reaction: $ {{H}_{2}}+{{I}_{2}}\xrightarrow[{}]{{}}2HI, $ the differential rate law is:
Jamia
Jamia 2005
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} $
Solution:
Correct answer is (b) $ -2\frac{d[{{H}_{2}}]}{dt}=-2\frac{d[{{I}_{2}}]}{dt}=\frac{d[HI]}{dt} $