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For a decomposition reaction the values ...

For a decomposition reaction the values of rate constant k at two different temperatures are given below :
`K_(1)=2.15xx10^(-8)L"mol"^(-1)s^(-1)"at " 650K`
`K_(2)=2.39xx10^(-7)L"mol"^(-1)s^(-1)"at " 700K`
Calclate the value of activation energy for this reaction.
`(R=8.314JK^(-1)"mol"^(-1))`

Text Solution

AI Generated Solution

To calculate the activation energy (Ea) for the given decomposition reaction, we can use the Arrhenius equation in its logarithmic form: \[ \log \frac{k_2}{k_1} = \frac{E_a}{2.303R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right) \] ### Step-by-step Solution: ...
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