For a first order reaction A → B:

k₁ = 1.24 x 10^-5 s^-1 at T₁ = 370 K

and k₂ = 5.36 x 10^-3 s^-1 at T₂ = 650 K

Determine the activation energy of this reaction.

Question

For a first order reaction A → B:

k₁ = 1.24 x 10^-5 s^-1 at T₁ = 370 K

and k₂ = 5.36 x 10^-3 s^-1 at T₂ = 650 K

Determine the activation energy of this reaction.

| General Chemistry 3

Accepted Answer

ln $\frac{k_{2}}{k_{1}}$ = $\frac{E_{a}}{R}$ x $(\frac{1}{T_{1}} - \frac{1}{T_{2}})$

Ea = R ln $\frac{k_{2}}{k_{1}}$ x $\frac{T_{1} T_{2}}{T_{2} - T_{1}}$

Ea = 8.314 x ln $(\frac{5.36 \times 10^{- 3}}{1.24 \times 10^{- 5}})$ x $\frac{370 \times 650}{280}$

Ea = 4.33 x 10⁴ J.mol^-1

Final - Question 10 | General Chemistry 3