# Problem: The decomposition of NH3 to N2 and H2 was studied on two surfaces:Without a catalyst, the activation energy is 335 kJ/mol.a. Which surface is the better heterogeneous catalyst for the decomposition of NH3? Why?b. How many times faster is the reaction at 298 K on the W surface compared with the reaction with no catalyst present? Assume that the frequency factor A is the same for each reaction.c. The decomposition reaction on the two surfaces obeys a rate law of the formRate = k [NH3] / [H2]How can you explain the inverse dependence of the rate on the H2 concentration?

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###### FREE Expert Solution

The decomposition reaction on the two surfaces obeys a rate law of the form

Rate = k [NH3] / [H2]

The decomposition reaction is an equilibrium reaction:

2 NH3 ⇌ N2 + 3 H2 ###### Problem Details

The decomposition of NH3 to N2 and H2 was studied on two surfaces: Without a catalyst, the activation energy is 335 kJ/mol.

a. Which surface is the better heterogeneous catalyst for the decomposition of NH3? Why?
b. How many times faster is the reaction at 298 K on the W surface compared with the reaction with no catalyst present? Assume that the frequency factor A is the same for each reaction.

c. The decomposition reaction on the two surfaces obeys a rate law of the form

Rate = k [NH3] / [H2]

How can you explain the inverse dependence of the rate on the H2 concentration?