The activation energy for the following reaction is 60. kJ/mol. Sn²⁺ + 2Co³⁺→ Sn⁴⁺ + 2Co²⁺
By what factor will the rate constant increase when the temperature is raised from 10°C to 28°C? (R = 8.314 J/mol• K)

Question

Quizplus · Accepted Answer

The rate constant's change with temperature can be calculated using the Arrhenius equation: $k = A e^{-E_a/(RT)}$, where $E_a$ is the activation energy, $R$ is the gas constant, and $T$ is the temperature in Kelvin. The ratio of the rate constants at two different temperatures (T2 and T1) is given by $\frac{k_2}{k_1} = e^{E_a/R(1/T_1 - 1/T_2)}$. Converting temperatures from Celsius to Kelvin (10°C = 283K, 28°C = 301K) and substituting the given values ($E_a = 60000 J/mol$, $R = 8.314 J/mol•K$), we find the factor by which the rate constant increases. Calculation yields a factor close to 4.6, indicating that the rate constant increases by approximately 4.6 times when the temperature is raised from 10°C to 28°C.

The Activation Energy for the Following Reaction Is 60