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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 decomposition reaction using the given rate constants (k1 and k2) at two different temperatures (T1 and T2), we can use the Arrhenius equation in its logarithmic form. ### Step-by-Step Solution: 1. **Write the Arrhenius Equation**: The Arrhenius equation is given by: \[ k = A e^{-\frac{E_a}{RT}} ...
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