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Consider the reaction : 2H(2)(g)+2NO(g...

Consider the reaction :
`2H_(2)(g)+2NO(g)rarrN_(2)(g)+2H_(2)(g)`
The rate law for this reaction is :
Rate = `k[H_(2)][NO]^(2)`
Under what conditions could these steps represent mechanism?
`{:("Step 1:",2NO(g)hArrN_(2)O_(2)(g)),("Step 2:",N_(2)O_(2)+H_(2)rarrN_(2)O+H_(2)O),("Step 3:",N_(2)O+H_(2)rarrH_(2)O+N_(2)):}`

A

These steps can never satisfy the rate law

B

Step 1 should be the slowest step

C

Step 2 should be the slowest step

D

Step 3 should be the slowest step

Text Solution

Verified by Experts

The correct Answer is:
C
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