The activation energy for a reaction is 84.0kJ/mol. Addition of a catalyst lowers the activation energy by 23.0 kJ/mol, while leaving the A-factor unchanged. By what factor ( uncatalyzed catalyzed k k ) does the rate increase at 25 °C?

Answer : The rate constant of the reaction is increased by factor,

Solution :

According to the Arrhenius equation,

The expression used with catalyst and without catalyst is,

where,

= rate of reaction with catalyst

= rate of reaction without catalyst

= activation energy with catalyst  = 23.0 kJ/mol = 23000 J/mol

= activation energy without catalyst  = 84.0 kJ/mol = 84000 J/mol

R = gas constant = 8.314 J/mol.K

T = temperature =

Now put all the given values in this formula, we get

Therefore, the rate constant of the reaction is increased by factor,

1.solid

2.carbon dioxide

3.helium

c. electrical charges of ionic bonds.