Question

From the following rate constants, determined at five temperatures, calculate the experimental energy of activation and ΔG^±,ΔH^±,andΔS^±for the reaction at 30°C:

Short answer

We have to findΔG^o, ΔH^o, ΔS^o

ΔG^o = 2.10 kcal/mol

ΔH° = 15.8 kcal/mol

ΔS° = 45 cal/(mol deg)

Step-by-step solution

Determining Ea

E_acan be determined from Arrhenius equation (ln k = - E_a/RT) because a plot of ln k versus 1/T gives a slope - E_a/R

Slope = -8290

E_a= -(slope)R

E_a= -(-8290)×1.98×10^-3 kcal/mol

E_a=16.4 kcal/mol

Step 2: To find ΔGo, ΔHo, ΔSo