Question

Calculate the activation energy, a , in kilojoules per mole for a reaction at 54.0 ∘C that has a rate constant of 0.272 s−1 and a frequency factor of 5.56×1011 s−1 . a=

Answer 1

To calculate the activation energy, use the Arrhenius equation and rearrange it to solve for Ea. Plug in the given values and convert units if necessary.

Step-by-step explanation:

The activation energy of a chemical reaction can be calculated using the Arrhenius equation with given values. The activation energy is found by rearranging this equation to solve for activation energy, substitifying given values and converting the result to kilojoules per mole.

To calculate the activation energy, we can use the Arrhenius equation:

k = Ae-Ea/RT

Given that the rate constant (k) is 0.272 s-1, the frequency factor (A) is 5.56x1011 s-1, and the temperature (T) is 54.0 °C (which needs to be converted to Kelvin), we can rearrange the equation to solve for activation energy (Ea) as follows:

Ea = -RT ln(k/A)

Plugging in the values, we get:

Ea = -8.314 J/mol K * (54.0 + 273.15) K * ln(0.272/5.56x1011)

Calculating this expression will give us the activation energy in joules per mole. To convert it to kilojoules per mole, we need to divide by 1000.

Learn more about activation energy