For a reaction, the activation energy is zero. What is the value of rate constant at `300 K` if `k=1.6 xx 10^(6)s^(-1)` at 280 K `(R= 8.31 JK^(-1)mol^

Question

For a reaction, the activation energy is zero. What is the value of rate constant at `300 K` if `k=1.6 xx 10^(6)s^(-1)` at 280 K `(R= 8.31 JK^(-1)mol^

For a reaction, the activation energy is zero. What is the value of rate constant at `300 K` if `k=1.6 xx 10^(6)s^(-1)` at 280 K
`(R= 8.31 JK^(-1)mol^(-1))`?

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

According to Arrhenius equation.
`logk_(2)/k_(1) = E_(a)/(2.303 R)[1/T_(1)-1/T_(2)] = 0/(2.303R) [ (T_(2)-T_(1))/(T_(1)T_(2))]=0`
`k_(2)/k_(1)` = Antilog = 0 = 1 or `k_(2) = k_(1) = 1.6 xx 10^(6)s^(-1)`

4 views Answered 2023-02-05 15:29