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For the decomposition of HI the followin...

For the decomposition of `HI` the following logarithmic plot is
shown `: [R=1.98 cal// mol - K]`

The activation energy of the reaction is about

A

`45600 cal`

B

`13500 cal`

C

`24600 cal`

D

`32300 cal`

Text Solution

Verified by Experts

The correct Answer is:
1
`logk=-(E_(a))/(2.303R)(1)/(T)+"constant"=-(E_(a))/(2.303R)xx10^(-3)xx(10^(3))/(T)+"constant"`
Thus slope of graph will be `-(E_(a)xx10^(-3))/(2.303R)= -(4)/(0.4)`
`implies" "E_(a)=2.303xx1.98xx10^(4)=45600cal`
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