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Activation Energy

The energy of...

Question

The energy of activation for a first order reaction is $104 k J m o l^{- 1}$ . The rate constant at $25^{o} C$ is $3.7 \times 10^{- 5} s^{- 1}$ . What is the rate constant at $30^{o} C$ ?

5.2 \times 10^{- 4} s^{- 1}

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7.4 \times 10^{- 5} s^{- 1}

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7.72 \times 10^{- 5} s^{- 1}

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None of these

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Solution

The correct option is C $7.4 \times 10^{- 5} s^{- 1}$
$l o g \frac{k_{2}}{k_{1}}$ = $\frac{E_{a}}{2.303 \times R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

Substituting the values,

$l o g \frac{k_{2}}{3.7 \times 10^{- 5}}$ = $\frac{104 \times 10^{3}}{8.314 \times 2.303} (\frac{1}{298} - \frac{1}{303})$

$k_{2} = 7.4 \times 10^{- 5} s^{- 1}$

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The energy of activation for a first order reaction is 104kJmol−1. The rate constant at 25oC is 3.7×10−5s−1. What is the rate constant at 30oC ?

The correct option is C 7.4×10−5s−1logk2k1 = Ea2.303×R(1T1−1T2)Substituting the values,logk23.7×10−5 = 104×1038.314×2.303(1298−1303)k2=7.4×10−5 s−1

The energy of activation for a first order reaction is $104 k J m o l^{- 1}$ . The rate constant at $25^{o} C$ is $3.7 \times 10^{- 5} s^{- 1}$ . What is the rate constant at $30^{o} C$ ?