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For the reaction:2 H2 + 2 NO → N2 + 2 H2Othe observed rate expression, under some conditions, is:rate = k[H2][NO]Which of the following mechanisms are consistent with these data?Select all that are True.step 1 2 NO → N2O2 (slow) step 2 N2O2 + H2 → N2O + H2O (fast) step 3 N2O + H2 → N2 + H2O (fast)step 1 NO + NO ⇌ N2O2 (fast) step 2 N2O2 + H2 → N2 + H2O + O (slow) step 3 O + H2 → H2O (fast)step 1 2 NO ⇌ N2O2 (fast) step 2 N2O2 + H2 → N2O + H2O (slow) step 3 N2O + H2 → N2 + H2O (fast)step 1 H2 + 2 NO → N2O + H2O (slow) step 2 N2O + H2 → N2 + H2O (fast)

Respuesta :

Answer:

The correct mechanism for the reaction based on the given rate is:

Step 1 : [tex]H_{2} +2NO->N_{2}O+H_{2}O(slow)[/tex]

Step 2: [tex]2N_{2}O+H_{2} ->N_{2}+H_{2}O(fast)[/tex]

Explanation:

The reaction rate of a muti-step reaction is determined by the slowest step of the reaction. Because of this reason, it is known as the rate-determining step of the reaction.

[tex]rate = k[H_{2}][NO][/tex]

The given rate expression has the concentrations of [tex]H_{2} , NO[/tex].

This means that the slowest step of the mechanism must involve [tex]H_{2} ,NO[/tex].

Among the proposed mechanisms, this criterion is met in the mechanism:

[tex]Step 1 :H_{2} +2NO->N_{2}O+H_{2}O(slow)\\ Step 2:2N_{2}O+H_{2} ->N_{2}+H_{2}O(fast)[/tex]

( Reason: In the above mechanism the slowest step involves [tex]H_{2} ,NO[/tex]. )

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