The activation energy for the following reaction is 60. kJ/mol.Sn²⁺ + 2Co³⁺ $\rarr$ Sn⁴⁺ + 2Co²⁺ By what factor (how many times) will the rate constant increase when the temperature is raised from 10^$\circ$C to 28^$\circ$C

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Quizplus · Accepted Answer

The rate constant's change with temperature can be calculated using the Arrhenius equation, which is $ k = A \exp\left(-\frac{E_a}{RT}\right) $, where $E_a$ is the activation energy, $R$ is the gas constant (8.314 J/mol·K), and $T$ is the temperature in Kelvin. The factor by which the rate constant increases can be found by taking the ratio of the rate constants at the two temperatures. Given the activation energy (60 kJ/mol = 60000 J/mol) and the temperatures (10°C = 283.15K and 28°C = 301.15K), the factor is approximately 4.6 when calculated.

The Activation Energy for the Following Reaction Is 60 →\rarr→ Sn4+ + 2Co2+ by What Factor (How Many Times) Will

The Activation Energy for the Following Reaction Is 60 $\rarr$ Sn⁴⁺ + 2Co²⁺ by What Factor (How Many Times) Will