What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from 300 K to 400 K ? (R = 8.314 J mol-1 K-1)

Question

What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from 300 K to 400 K ? (R = 8.314 J mol-1 K-1) (A) 69.8 (B) 6.92 (C) 34.4 (D) 3.44

Tardigrade Admin · Accepted Answer

log (K2/K1)=(Ea/2.3R)((1/T1)-(1/T2)) log (2/1)=(Ea/2.33×8.31) ((1/300)-(1/400)) = 0.3 x 2.3 x 8.31 x 3 x 400 = Ea Ea = 6.88 kJ

Q. What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from 300 K to 400 K ? (R = 8.314 J $m o l^{- 1} K^{-} 1$ )

69.8

6.92

34.4

3.44

log $\frac{K _{2}}{K _{1}} = \frac{E _{a}}{2.3 R} (\frac{1}{T _{1}} - \frac{1}{T _{2}})$
log $\frac{2}{1} = \frac{E _{a}}{2.33 \times 8.31} (\frac{1}{300} - \frac{1}{400})$
= 0.3 x 2.3 x 8.31 x 3 x 400 = E_a
E_a = 6.88 kJ

Q. What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from 300 K to 400 K ? (R = 8.314 J mol−1K−1)