Question

The basic theory behind Arrhenius equation is that:

• A. The number of effective collision is proportional to the number of molecules above a certain threshold energy.
• B. As the temperature increases, so does the number of molecules with energies exceeding the threshold energy.
• C. The rate constant is a function of temperature.
• D. The activation energy and pre-exponential factor are always temperature independent.

Answer 1

Answer: (A), (B), (C), (D)

The correct options are
A The number of effective collision is proportional to the number of molecules above a certain threshold energy.
B As the temperature increases, so does the number of molecules with energies exceeding the threshold energy.
C The rate constant is a function of temperature.
D The activation energy and pre-exponential factor are always temperature independent.

As we know, higher the temperature, the faster a given chemical reaction will proceed. Quantitatively, this relationship between the rate a reaction proceeds and its temperature is determined by the Arrhenius Equation. At higher temperatures, the probability that two molecules will collide is higher. This higher collision rate results in a higher kinetic energy, which has an effect on the activation energy of the reaction. The activation energy is the amount of energy required to ensure that a reaction happens.

This calculator calculates the effect of temperature on reaction rates using the Arrhenius equation.

$k=A{e}^{-E_a/RT}$, where k is the rate coefficient, A is a constant, Ea is the activation energy, R is the universal gas constant, and T is the temperature (in kelvin).

Here, activation energy and pre-exponential factor are always temperature independent.

So, rate constant is a function of temperature.