The reaction (CH3) 3CBr + OH - (CH3) 3COH + Br - in a certain solvent is first order with respect to (CH3) 3CBr and zero order with respect to OH-. In several experiment, the rate constant k was determined at different temperatures. A plot of ln (k) versus 1/T was constructed resulting in a straight line with a slope value of - 1.10 x 104 K and a y-intercept of 33.5.

Answer and Explanation:

The rate constant (K) is related to activation energy (Ea), frequency factor (A) and temperature (T) in Kelvin by the equation

R = molar gas constant

K = A (e^ (-Ea/RT))

Taking natural log of both sides

In K = In A - (Ea/RT)

In K = (-Ea/R) (1/T) + In A

Comparing this to the equation of a straight line; y = mx + c

y = In K, slope, m = (-Ea/R), x = (1/T) and intercept, c = In A

a) From the question, m = (-Ea/R) = - 1.10 * (10^4) K

(-Ea/R) = - 1.10 * (10^4) = - 11000

R = 8.314 J/K. mol

Ea = - 11000 * 8.314 = 91454 J/mol = 91.454 KJ/mol

b) c = In A = 33.5

A = e^33.5 = (3.54 * (10^14)) / s

c) K = A (e^ (-Ea/RT))

A = (3.54 * (10^14)) / s, Ea = 91454 J/mol, T = 25°C = 298.15 K, R = 8.314 J/K. mol

K = (3.54 * (10^14)) (e^ (-91454 / (8.314*298.15))) = 0.0336/s

QED!