If the temperature in problem 16.60 (25C), by what factor does the fraction of collisions with energy equal to or greater that the activation energy change?

What is the Ea change?

To determine the factor by which the fraction of collisions with energy equal to or greater than the activation energy changes when the temperature increases, we need to consider the Arrhenius equation.

The Arrhenius equation relates the rate constant of a chemical reaction to temperature and activation energy. It is given by:

k = Ae^(-Ea/RT)

Where:
- k is the rate constant
- A is the pre-exponential factor or the frequency factor
- Ea is the activation energy
- R is the gas constant
- T is the temperature in Kelvin

In this case, we need to compare the fraction of collisions with energy equal to or greater than the activation energy at two different temperatures, T1 and T2. Let's assume T1 is the initial temperature, given as 25°C, which needs to be converted to Kelvin.

T1 = 25°C + 273.15 = 298.15 K

Now, let's assume T2 is the new temperature after the change. We are given that the temperature is 25°C, so we'll convert it to Kelvin as well:

T2 = 25°C + 273.15 = 298.15 K

Since T1 and T2 are the same, the factor by which the fraction of collisions with energy equal to or greater than the activation energy changes is 1.

Therefore, the fraction of collisions with energy equal to or greater than the activation energy does not change when the temperature is 25°C.