The gas phase reaction 2 N2O5(g) → 4 NO2(g) + O2(g) has an activation energy of 103 kJ/mol, and the first order rate constant is 1.35×10-5 min-1 at 266 K. What is the rate constant at 296 K?

 The rate constant at 296 K is

Explanation:

According to the Arrhenius equation,

or,

where,

= rate constant at 266 K =

= rate constant at 296 K = ?

= activation energy for the reaction = 103 kJ/mol = 103000 J/mol

R = gas constant = 8.314 J/mole.K

= initial temperature = 266 K

= final temperature = 296 K

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

Thus the rate constant at 296 K is

2b2t

explanation:

2b2t