A rate constant obeys the Arrhenius equation, the factor A being 2.2 ×10¹³ s^-1 and the activation energy being 150. kJ mol^-1. What is the value of the rate constant at 227°C, in s^-1?

Question

Quizplus · Accepted Answer

The Arrhenius equation is:k = A * exp(-Ea/RT)where:k is the rate constantA is the pre-exponential factorEa is the activation energyR is the gas constant (8.314 J/mol*K)T is the temperature in KelvinWe are given:A = 2.2 × 10^13 s^-1Ea = 150 kJ/mol = 150,000 J/molT = 227°C + 273.15 = 500.15 KPlugging these values into the Arrhenius equation, we get:k = 2.2 × 10^13 s^-1 * exp(-150,000 J/mol / (8.314 J/mol*K * 500.15 K))k = 2.2 × 10^13 s^-1 * exp(-36.02)k = 2.2 × 10^13 s^-1 * 4.7 × 10^-16k = 1.03 × 10^-2 s^-1Therefore, the value of the rate constant at 227°C is 1.03 × 10^-2 s^-1, which is closest to choice D) 4.7 × 10^-3 s^-1.

A Rate Constant Obeys the Arrhenius Equation, the Factor a Being