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At high pressure the following reaction is zero order.
\[
2 \mathrm{NH}_{3}(\mathrm{~g}) \stackrel{1130 \mathrm{~K}}{\text { Platinum catalyst }} \mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g})
\]
\( \mathrm{P} \)
Which of the following options are correct for this reaction?
W
(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.
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