The decomposition of ammonia on platinum surface follow the change, 2 NH _3 N _2 + 3 H _2

CHEMISTRY · Multi-part · AP · Chemistry · Kinetics · Kinetics

Problem

The decomposition of ammonia on platinum surface follow the change, 2NH3⟶N2+3H22\text{NH}_3 \longrightarrow \text{N}_2 + 3\text{H}_2 (a) What does −d[NH3]dt\frac{-d[\text{NH}_3]}{dt} denote? (b) What does d[N2]dt\frac{d[\text{N}_2]}{dt} and d[H2]dt\frac{d[\text{H}_2]}{dt} denote? (c) If the decomposition is zero order then what are the rate of production of N2\text{N}_2 and H2\text{H}_2 , if K=2.5×10−4 M s−1K = 2.5 \times 10^{-4} \text{ M s}^{-1} ? (d) If the rate obeys −d[NH3]dt=K1[NH3]1+K2[NH3]-\frac{d[\text{NH}_3]}{dt} = \frac{K_1[\text{NH}_3]}{1 + K_2[\text{NH}_3]} , what will be the order for decomposition of NH3\text{NH}_3 , if (i) [NH3][\text{NH}_3] is very very less and (ii) [NH3][\text{NH}_3] is very very high? K1K_1 and K2K_2 are constants.

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