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Question
At high pressure the following reaction is zero order.
\[\ce{2NH3(g) ->[1130 K][Platinum catalyst] N2(g) + 3H2(g)}\]
Which of the following options are correct for this reaction?
(i) Rate of reaction = Rate constant.
(ii) Rate of the reaction depends on concentration of ammonia.
(iii) Rate of decomposition of ammonia will remain constant until ammonia disappears completely.
(iv) Further increase in pressure will change the rate of reaction.
Solution
(i) Rate of reaction = Rate constant.
(iii) Rate of decomposition of ammonia will remain constant until ammonia disappears completely.
(iv) Further increase in pressure will change the rate of reaction.
Explanation:
The pressure in this reaction is extremely high and it becomes independent of the ammonia concentration. The metal surface becomes saturated with gas molecules when the rate of reaction = Rate constant. The rate of a zero-order reaction is independent of the concentration of reactants in the reaction.
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