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?

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The Arrhenius equation is: k = A * exp(-Ea/RT)where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant (8.314 J/mol*K), and T is the temperature in Kelvin.Plugging in the given values, we get: k = 2.2 × 10^13 s^-1 * exp(-150000 J/mol / (8.314 J/mol*K * 500 K)) = 4.7 × 10^-3 s^-1

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