I would use the Arrhenius equation, Ea = 125 kJ/mol, T1 = 273, T2 = 293, k1 = a convenient number such as 10, solve for k2. Then do the same but this time make Ea 125 kJ/mol (remember to change to J/mol in the Arrhenius equation), and re-solve for k2. Then you can find the factor between the two values for k2.
b is done the same way.
The presence of a catalyst provides a reaction pathway in which the activation energy of a certain reaction is reduced from 125 kJ·mol-1 to 75 kJ·mol-1.
(a) By what factor does the rate of the reaction increase at 293 K, all other factors being equal?
(b) By what factor would the rate change if the reaction were carried out at 339 K instead?
1 answer
0 answers