Chemistry, 07.03.2020 02:48 gizmo50245
He rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy . If the rate constant of this reaction is at , what will the rate constant be at ?
Answers: 2
![\ln(\frac{K_{324^oC}}{K_{244^oC}})=\frac{E_a}{R}[\frac{1}{T_1}-\frac{1}{T_2}]](/tpl/images/0537/2208/1ff41.png)
= equilibrium constant at 244°C = 
= equilibrium constant at 324°C = ?
= Activation energy = 71.0 kJ/mol = 71000 J/mol (Conversion factor: 1 kJ = 1000 J)
= initial temperature = ![244^oC=[273+244]K=517K](/tpl/images/0537/2208/c11e6.png)
= final temperature = ![324^oC=[273+324]K=597K](/tpl/images/0537/2208/4d511.png)
![\ln(\frac{K_{324^oC}}{6.7})=\frac{71000J}{8.314J/mol.K}[\frac{1}{517}-\frac{1}{597}]\\\\K_{324^oC}=61.29M^{-1}s^{-1}](/tpl/images/0537/2208/108e2.png)
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