Step1the following mechanism has been proposed for the reaction of NO with H2 to

ID: 532379 • Letter: S

Question

Step1the following mechanism has been proposed for the reaction of NO with H2 to form N20 and H20

STEP 1 N0 g + No g left @ right arrow N2O2 g fast

step 2 N2O2g +H2 right arrow N2Og + H2O g slow

Write the overall reaction

write the rate law forc each elementry resaction in the mechanism

step1 rate =

step2 rate =

identify any intermediates in the mechanism

what is the rate law according to the mechanism

Step1the following mechanism has been proposed for the reaction of NO with H2 to form N20 and H20

STEP 1 N0 g + No g <-----> N2O2 g fast

for the above step, -rNO= K1[NO][NO]- K-1[N2O2](1), K1 and K-1 are rate constants for the forward and backward reactions.

step 2 N2O2g +H2----> N2Og + H2O (g) slow (2)

for the step2, -N2O2= K2[N2O2] [H2] , K2 is the rate constant for the second reaction.

The intermediate is [N2O2]. The slowest step in a series of elementary reactions will be the rate limitng step.

Hence rate = K2[N2O2][H2]

from Eq.1, since fast and Equlibrium is established, the net rate of intermediate is zero. i.e rN2O2=0

K1[NO] [NO]- K-1[N2O2]=0 and [N2O2]= K1[NO]2/ K-1

hence rate = K2 K1[NO]2 [H2]/K-1 = K' [NO]2 [H2] where K'= K2K1/K-1

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