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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))`

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To calculate the activation energy (Ea) for the given decomposition reaction using the Arrhenius equation, we can follow these steps: ### Step 1: Write down the given data - Rate constant at 650 K: \( K_1 = 2.15 \times 10^{-8} \, L \, mol^{-1} \, s^{-1} \) - Rate constant at 700 K: \( K_2 = 2.39 \times 10^{-7} \, L \, mol^{-1} \, s^{-1} \) - Temperature 1: \( T_1 = 650 \, K \) - Temperature 2: \( T_2 = 700 \, K \) - Universal gas constant: \( R = 8.314 \, J \, K^{-1} \, mol^{-1} \) ...
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