Question
The decomposition of ammonia on a platinum surface at 1129 K occurs according to the following...
The decomposition of ammonia on a platinum surface at 1129 K occurs according to the following reaction: 2 NH3(g) --> N2(g) + 3 H2(g). It occurs via zero order kinetics. Use the following kinetic data which report the variation of ammonia concentration in the gas phase with time "t" to evaluate the rate constant for the reaction at 1129 K.
| 103[NH3] (in M) | 2.10 | 1.85 | 1.47 | 1.23 | .86 | .57 | .34 |
| t/s | 0 | 200 | 400 | 600 | 800 | 1000 | 1200 |
Suggest why the reaction exhibits zero order kinetics with respect to the concentration of ammonia in the gas phase.
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