Chemistry, 21.04.2020 18:50 xxaurorabluexx
For the second-order reaction NO( g) + O 3( g) → NO 2( g) + O 2( g), the rate constant has been measured to be 1.08 × 10 7 M –1 s –1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K. What is the rate constant at 207 K? ( R = 8.3145 J K –1 mol –1)
Answers: 1
![\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]](/tpl/images/0615/2426/6d953.png)
= rate constant at 
= 
= rate constant at 
= ?
= activation energy for the reaction = 
= initial temperature = 298 K
= final temperature = 207 K![\log (\frac{K_2}{1.08\times 10^7M^{-1}s^{-1}})=\frac{11400J/mol}{2.303\times 8.314J/mole.K}[\frac{1}{298K}-\frac{1}{207K}]](/tpl/images/0615/2426/e96a1.png)
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For the second-order reaction NO( g) + O 3( g) → NO 2( g) + O 2( g), the rate constant has been meas...
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