Requirement 1:
22
NO Cl NO Cl Cl
Cl NO NO Cl
NO Cl NO Cl
22 2
22
22 2
"
"
"
++
+
+
Requirement 2:
NO 2 (g) + Cl 2 (g) →NO 2 C1 + Cl
is the rate-determining step. This step is bimolecular.
rate = k 1 [NO 2 ][Cl 2 ]
as found in part (a).
Meeting these two requirements does not prove that this isthe mechanism for the
reaction — only that it could be.
- Hydrogen peroxide, H 2 O 2 , decomposes by first-order decomposition and has a rate
constant of 0.015/min at 200°C. Starting with a 0.500 M solution of H 2 O 2 , calculate:
(a) The molarity of H 2 O 2 after 10.00 min
(b) The time it will take for the concentration of H 2 O 2 to go from 0.500 M to
0.150 M
(c) The half-life
Answer
- Given: H 2 O 2 , first-order decomposition
k= 0.015/min at 200°C
[H 2 O 2 ] 0 = 0.500 M
(a) Restatement: Calculate [H 2 O 2 ] after 10.00 min.
For first-order reactions: rate = kX →−dX/dt= kX
Integrating from X 0 to Xgives
ln XX kt
0
-=cm
log X.
Xkt
230
cm^0 =
log..
X
cm0 500M =0 065
.
X
0 500= 10 0 065.
..
X
0 500= 12
.
X.. M
12
==0 500 042
Kinetics