Question

the energy of activation for a reaction is 105kj/mil.calculate the specific rate for a reaction at 300K,if the frequency factor is 2.5×10power15 per second​

Answer 1

Answer:

A=(10.9634)=9.914×10  

10

Explanation:

By using arrhenius equation,

⟹logk=  

2.303 RT

−E  

a

​

 

​

+logA

We get

⟹logA=log(1.8×10  

−5

)+  

2.303×8.314×313

94140

​

 

⟹(log1.8)−5+15.7082)

⟹0.2553−5+15.7082=10.9635

∴logA=(10.9634)=9.914×10  

10