The decomposition of NH3 to N2 and H2 was studied on two surfaces:
Surface E a (kJ/mol)
Without a catalyst, the activation energy is 335 kJ/mol.
How many times faster is the reaction at 275. K on the W surface compared with the reaction with no catalyst present? Assume the frequency factor A is the same for each reaction.
set up a ratio of the Arrhenius equations and solve for the ratio of rate constants.
How can we set up a ratio if the concentration is unknown? even if it was the same, won't that affect the ratio? I tried to solve it ignoring the concentration and it didn't work.