The activation energy of a certain reaction is 65.7 kJ/mol. How many times faster will the reaction occur at 51°C than at 8°C?
State the assumptions you need to make in order to perform this calculation. (Select all that apply.)
The collision model and the Arrhenius equation describe the kinetics of the reaction.
The frequency factor is constant over the temperature range. Initial concentrations are the same at the two temperatures.
Activation energy is constant over the temperature range.
The rate constants are inversely proportional to the temperature range.
I do not know myself sorry
In order to calculate how many times faster a reaction occurs at a higher temperature compared to a lower temperature, we can use the Arrhenius equation. The Arrhenius equation describes the relationship between the rate constant (k) and the temperature (T) of a chemical reaction.
The Arrhenius equation is given by:
k = A * exp(-Ea / (R * T))
Where:
k is the rate constant
A is the frequency factor
Ea is the activation energy
R is the gas constant (8.314 J/(mol·K))
T is the temperature in Kelvin (K)
To calculate the ratio of reaction rates at two different temperatures, we need to assume that the frequency factor (A) and the activation energy (Ea) remain constant over the temperature range. Additionally, we assume that the initial concentrations are the same at the two temperatures.
Answer: The assumptions that need to be made in order to perform this calculation are:
- The frequency factor (A) is constant over the temperature range.
- Initial concentrations are the same at the two temperatures.
- Activation energy (Ea) is constant over the temperature range.
- The rate constants (k) are inversely proportional to the temperature range.