1)The following proposed mecchanism for the reaction A + B= C + D: Step 1: A + C

Question

1)The following proposed mecchanism for the reaction A + B= C + D: Step 1: A + C = 2D (slow) ; Step 2: B + D = 2C (fast). The rate law consistent with this mechanism would be:_______________. 2) Consider the proposed mechanism for the reaction between nitrogen monoxide and chlorine: Step 1: NO + Cl2= NOCl2 (fast); Step 2: NOCl2 + NO = 2 NOCl (slow). The reaction intermediate in this mechanism is________________. 3) NO2= NO + O and O2 + O = O3 a) The reaction intermediate for this mechanism is___________ b) The reactants of this reaction are ______________.

Explanation / Answer

1)The following proposed mecchanism for the reaction A + B= C + D: Step 1: A + C = 2D (slow) ; Step 2: B + D = 2C (fast).

rate law depends on the slowest step

here 1st step is the slowest step

so, rate law is:

rate = k [A][C]

2) Consider the proposed mechanism for the reaction between nitrogen monoxide and chlorine: Step 1: NO + Cl2= NOCl2 (fast); Step 2: NOCl2 + NO = 2 NOCl (slow).

NOCl2 is produced in step 1 and used up in step 2.

So, NOCl2 is intermediate

3) NO2= NO + O and O2 + O = O3

a) O is produced in step 1 and used up in step 2.

So, O is intermediate

b) Lets add both steps to get overall reaction

NO2 + O2 —> NO + O3

NO2 and O2 are reactants

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