The activation energy for a reaction at temperature T K was found to be or `2.303 "RT J mol"^(-1)`. The ratio of the rate constant to Arrhenius factor

Question

The activation energy for a reaction at temperature T K was found to be or `2.303 "RT J mol"^(-1)`. The ratio of the rate constant to Arrhenius factor

The activation energy for a reaction at temperature T K was found to be or `2.303 "RT J mol"^(-1)`. The ratio of the rate constant to Arrhenius factor is
A. 0.01
B. 0.1
C. 0.02
D. 0.001

Monjur Alahi

4 views

2025-01-04 04:42

1 Answers

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Salim Ahmed Kawsar · Accepted Answer · 2023-02-05T15:29:48+06:00

Salim Ahmed Kawsar

Correct Answer - B
log K=log `A -(E_(a))/(2.303RT)`
logK-log `A-(E_(a))/(2.303RT)`
log `((K)/(A))=(-2.303RT)/(2.303RT)=-1`
`(k)/(A)="antilog" (-1.0)=1xx10^(-1)=0.1`

4 views Answered 2023-02-05 15:29