Nitrogen monoxide reacts with hydrogen gas: H_2(g) + NO_(g) rightarrow products

Question

Nitrogen monoxide reacts with hydrogen gas: H_2(g) + NO_(g) rightarrow products One of many proposed mechanisms for the reaction is: step 1 H_2 + NO rightarrow H_2O + N (slow) step 2 N + NO rightarrow N_2 + O (fast) step 3 O + H_2 rightarrow H_2O (fast) Which statements, if any, about this mechanism are true? The mechanism predicts that the reaction is first order in H_2. The mechanism predicts that the reaction is second order in NO. The mechanism predicts that the reaction is third order overall. The mechanism predicts that oxygen atoms, O, are intermediates in the reaction. The mechanism predicts that nitrogen molecules, N_2 are intermediates in the reaction. The mechanism proposes a total of 2 distinct intermediates in the reaction. The first step of the mechanism has a lower energy of activiation than the second and third steps. The addition of a catalyst for the reaction to the reaction flask will change the mechanism.

Explanation / Answer

Solution:

Step 1 predicts the mechanism is first order, step 2 and 3 clearly shows oxygen molecule acts as intermediate from the fast reaction sequence. Step 1 to 3 shows two different intermediate molecules and also activation energy plays a role in mechanism step, slowest is the cause of higher activation energy and fast is of lower activation energy. The given reaction steps are of catalytic converter used in automobiles exhaust system.

Hence the option to be selected for the correct answer are 1,4,6 &7.

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