Chemistry, 29.01.2020 01:42 chasechevy13
Consider the reaction data. a ⟶ products a⟶products t ( k ) t (k) k ( s − 1 ) k (s−1) 225 225 0.391 0.391 525 525 0.700 0.700 what two points should be plotted to graphically determine the activation energy of this reaction? to avoid rounding errors, use at least three significant figures in all values.
Answers: 2
![\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]](/tpl/images/0479/5717/6d953.png)
= rate constant at 225 K = 
= rate constant at 525 K = 
= activation energy for the reaction = ?
![\log (\frac{0.700 s^{-1}}{0.391 s^{-1}})=\frac{Ea}{2.303\times 8.314J/mole.K}[\frac{1}{225 K}-\frac{1}{525 K}]](/tpl/images/0479/5717/85e41.png)
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Consider the reaction data. a ⟶ products a⟶products t ( k ) t (k) k ( s − 1 ) k (s−1) 225 225 0.391...
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