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  • The rate constant for the first order decomposition of  is given by the following equation: <img alt="\log k=14.2 -\frac{1.0\times 10^{4}

The rate constant for the first order decomposition of H_{2}O_{2} is given by the following equation:

\log k=14.2 -\frac{1.0\times 10^{4}}{T}

Calculate Ea for this reaction and rate constant k if its half - life period be 200 minutes. ( Given: R = 8.314 JK-1mol-1)

 

 

 

 

 
 
 
 
 

Answers (1)

E_{a}=?, k=?

R = 8.314 JK-1mol-1

t_{\frac{1}{2}}=200 min

\log k=14.2 -\frac{1.0\times 10^{4}}{T}

order = 1

\log K= \log A -\frac{E_{o}}{2.303T}

\frac{E_{a}}{2.303T}=\frac{1.0\times 10^{4}}{T}

E_{a}=1\times 10^{4}K\times 2.303 \times R

E_{a}= 2.303 \times10^{4} \times 8.314

E_{a}= 19.147142 \times 10^{4}

E_{a}= 19147.142Jmol^{-1}

t_{\frac{1}{2}}=200 min

K=\frac{0.693}{t_{\frac{1}{2}}}=\frac{0.693}{200}=0.003465min^{-1}=0.2079sec^{-1}

 

 

 

 

 

 

 

Posted by

Sumit Saini

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