The decomposition of NH3 on platinum surface is zero order reaction. What are the rates of production of N2 and H2 if Ar=2.5 x 10-4 mol-1 Ls-1.

The decomposition of NH3 (Ammonia) on a platinum surface is represented by the following balanced chemical equation:

2NH3 → N2 + 3H2

This is a zero order reaction, which means the rate of reaction is independent of the concentration of the reactants. The rate of reaction is given as Ar=2.5 x 10^-4 mol L^-1 s^-1.

The rate of production of N2 and H2 can be determined from the stoichiometry of the reaction.

For every 2 moles of NH3 that decompose, 1 mole of N2 and 3 moles of H2 are produced.

Therefore, the rate of production of N2 is the same as the rate of decomposition of NH3, which is 2.5 x 10^-4 mol L^-1 s^-1.

The rate of production of H2 is three times the rate of decomposition of NH3, because for every mole of NH3 that decomposes, three moles of H2 are produced. Therefore, the rate of production of H2 is 3 * 2.5 x 10^-4 mol L^-1 s^-1 = 7.5 x 10^-4 mol L^-1 s^-1.