Question

for a chemical reaction at 27°C, the activation energy is 600R. The ratio of the rate constants at 327°C to that of at 27°C will be​

Answer 1

• The ratio of rate constants at 327° C to that at 27° C is e.

Given-

• Activation energy of the chemical reaction = 600 R
• Initial temperature (T₁) = 27° C = 300 K
• Final temperature (T₂) = 327° C = 600 K

From the Arrhenius equation we can find out the ratio of rate constants -

ln ( K₂/K₁)  = Ea / R (1/T₁ - 1/T₂) ,

where Ea is the activation energy, R is the universal gas constant, K₁ is the rate constant at temperature T₁, and K₂ is the rate constant at temperature T₂.

Now by putting the values we get -

ln ( K₂/K₁) = 600 R/R ( 1/300 - 1/600)

ln ( K₂/K₁)  = 600 ( 2-1/600)

ln ( K₂/K₁)  = 1

So,  K₂/K₁ = e¹ = e

Hence ratio of rate constants is e .

Regards

Answer 2

Explanation:

hope this will help you