The activation energy of a certain uncatalysed reaction at 300 K is 76 k) per mole. The activation energy is lowered to 57 kJ per mole by the lise of a catalyst. By what factor is the rate of the catalysed reaction increased?

Explanation

To find the factor by which the rate of the catalyzed reaction is increased, we can use the Arrhenius equation and the relationship between the rate constants of the uncatalyzed and catalyzed reactions. The steps are as follows:

### Step 1: Identify the given values
- Activation energy of uncatalyzed reaction (Ea1) = 76 kJ/mol
- Activation energy of catalyzed reaction (Ea2) = 57 kJ/mol
- Temperature (T) = 300 K

### Step 2: Use the Arrhenius equation
...