The reaction c4h8(g)⟶2c2h4(g) c4h8(g)⟶2c2h4(g) has an activation energy of 262 kj/mol.262 kj/mol. at 600.0 k,600.0 k, the rate constant, , is 6.1×10−8 s−1.6.1×10−8 s−1. what is the value of the rate constant at 785.0 k?

Answer : The rate constant at 785.0 K is,

Explanation :

According to the Arrhenius equation,

or,

where,

= rate constant at =

= rate constant at = ?

= activation energy for the reaction = 262 kJ/mole = 262000 J/mole

R = gas constant = 8.314 J/mole.K

= initial temperature =

= final temperature =

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

Therefore, the rate constant at 785.0 K is,