What is the activation energy for a reaction it its rate doubles when the temperature is raised from 20° C to 35° C ? (R = 8.314 J mol-1 K-1)

Question

What is the activation energy for a reaction it its rate doubles when the temperature is raised from 20° C to 35° C ? (R = 8.314 J mol-1 K-1) (A) 15.1 kJ mol-1  (B) 342 kJ mol-1  (C) 269 kJ mol-1  (D) 34.7 kJ mol-1

Tardigrade Admin · Accepted Answer

log (k2/k1) = (Ea/2.303 × R) ((1/293) - (1/308)) log 2 = (Ea/2.303R) ((308 - 293/293 ×308)) Ea = 34673 J = 34.67 kJ

Q. What is the activation energy for a reaction it its rate doubles when the temperature is raised from $2 0^{\circ} C$ to $3 5^{\circ} C$ ? $(R = 8.314 J m o l^{- 1} K^{- 1})$

$15.1 k J m o l^{- 1}$

$342 k J m o l^{- 1}$

$269 k J m o l^{- 1}$

$34.7 k J m o l^{- 1}$

$lo g \frac{k _{2}}{k _{1}} = \frac{E a}{2.303 \times R} (\frac{1}{293} - \frac{1}{308})$
$lo g 2 = \frac{E a}{2.303 R} (\frac{308 - 293}{293 \times 308})$
$E_{a} = 34673 J = 34.67 k J$

Q. What is the activation energy for a reaction it its rate doubles when the temperature is raised from 20∘C to 35∘C ? (R=8.314Jmol−1K−1)

15.1kJmol−1

342kJmol−1

269kJmol−1

34.7kJmol−1