Question

If a temperature increase from 12. 0 °C to 20. 0 °C doubles the rate constant for a reaction. What is the value of the activation barrier for the reaction?

Answer 1

If a temperature increase from 12. 0 °C to 20. 0 °C doubles the rate constant for a reaction. What is the value of the activation barrier for the reaction is 60.155KJ/mol.

What is activation energy?

Activation energy is defined as the minimum amount of energy required by molecules to occur a chemical reaction. It is denoted by Ea.

Given,

T1 = 12+273 = 285K

T2 = 20 +273 = 293K

Rate constant = k2/k1 = 2:1

Using arrhenius equation which give relationship between constant of reaction and temperature is

In(k2/k1) = Ea/(R[1/T1 - 1/T2]

where, Ea is the activation energy

and R is the gas constant

T1 is the initial temperature

T2 is the final temperature

In2= Ea/R[(1/285) - (1/293)]

Ea = In2 × 8.314 ×285×293/8

Ea = 0.301 ×8.314 ×285×293/8

Ea = 60155J/mol

Ea = 60.155KJ/mol.

Thus we calculated that the activation energy for a reaction at 12°C to 20°C is 60.155KJ/mol.

learn more about activation energy:

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