Question

Calculate the activation energy, a , in kilojoules per mole for a reaction at 55 ∘C that has a rate constant of 0.201 s−1 and a frequency factor of 9.65×1011 s−1 . a= kJ/mol

Answer 1

The activation energy of the reaction was calculated using the rearranged Arrhenius equation and the given parameters. The activation energy in J/mol was then converted to kJ/mol.

Step-by-step explanation:

To calculate the activation energy of the reaction, we'll need to use the Arrhenius equation reorganized to solve for activation energy (Ea): Ea = -RTln(k/A), where R is the gas constant (8.314 J/mol/K), T is the absolute temperature in Kelvin, k is the rate constant and A is the frequency factor.

To convert the given temperature from Celsius to Kelvin, we add 273.15 to it, making it 328.15 K. Substituting these values into the equation, we get Ea = -8.314 * 328.15 * ln(0.201 / (9.65 × 1011)). Solving for Ea will give us the activation energy in J/mol. To convert the answer to kJ/mol, you divide the result by 1000.

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