The reaction between nitrogen dioxide and carbon monoxide is NO2(g)+CO(g)→NO(g)+CO2(g)NO2(g)+CO( g)→NO(g)+CO2(g) The rate constant at 701 KK is measured as 2.57 M−1⋅s−1M−1⋅s−1 and that at 895 KK is measured as 567 M−1⋅s−1M−1⋅s−1. The activation energy is 1.5×102 1.5×102 kJ/molkJ/mol. Predict the rate constant at 525 KK .

Answer : The rate constant at 525 K is,

Explanation :

According to the Arrhenius equation,

or,

where,

= rate constant at =

= rate constant at = ?

= activation energy for the reaction =

R = gas constant = 8.314 J/mole.K

= initial temperature = 701 K

= final temperature = 525 K

Now put all the given values in this formula, we get:

Therefore, the rate constant at 525 K is,