Chemistry, 26.02.2020 17:55, shadowselena63
The rate constant of a reaction is 6.85 × 10−5 L/mol·s at 195°C and 2.20 × 10−3 L/mol·s at 258°C. What is the activation energy of the reaction? Enter your answer in scientific notation.
Answers: 1
![\ln(\frac{K_{258^oC}}{K_{195^oC}})=\frac{E_a}{R}[\frac{1}{T_1}-\frac{1}{T_2}]](/tpl/images/0525/0415/d01a9.png)
= equilibrium constant at 258°C = 
= equilibrium constant at 195°C = 
= Activation energy of the reaction = ?
= initial temperature = ![195^oC=[195+273]K=468K](/tpl/images/0525/0415/d4d73.png)
= final temperature = ![258^oC=[258+273]K=531K](/tpl/images/0525/0415/697bf.png)
![\ln(\frac{2.20\times 10^{-3}}{6.85\times 10^{-5}})=\frac{E_a}{8.314J/mol.K}[\frac{1}{468}-\frac{1}{531}]\\\\E_a=113780J/mol=113.8kJ/mol](/tpl/images/0525/0415/e4c71.png)
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The rate constant of a reaction is 6.85 × 10−5 L/mol·s at 195°C and 2.20 × 10−3 L/mol·s at 258°C. Wh...
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