Answer:
Explanation:
The given overall reaction is as follows:
O
2
N
N
H
₂(
a
q
)
k
→
N
₂O
(
g
)
+
H
₂
O(
l
)
The reaction mechanism for this reaction is as follows:
O
₂
N
N
H
₂
⇌
k
1
k
−
1 O
₂N
N
H
⁻
+
H
⁺
(
f
a
s
t e
q
u
i
l
i
b
r
i
u
m
)
O
₂
N
N
H
−
k
₂→
N
₂
O
+
O
H
⁻
(
s
l
ow
)
H
⁺
+
O
H
−
k
₃→
H
₂
O
(
f
a
s
t
)
The rate law of the reaction is given as follows:
k
=
[
O
₂
N
N
H
₂
] / [
H
⁺
]
The rate law can be determined by the slow step of the mechanism.
r
a
t
e
=
k
₂
[
O
₂
N
N
H
⁻
]
.
.
.
(
1
)
Since, from the equilibrium reaction
k
e
q
=
[
O
₂
N
N
H
⁻
]
[
H
⁺
]
/[
O
₂
N
N
H
₂
]
=
k
₁
/k
−
1
[
O
₂
N
N
H
⁻]
=
k
₁
/k
−
1 ×
[
O
₂
N
N
H
₂
]
/[
H
⁺
].
.
.
.
(
2
)
Substitituting the value of equation (2) in equation (1) we get.
r
a
t
e
=
k
₂
k
₁/
k
−
1 ×
[
O
₂
N
N
H
₂
]
/[
H
⁺
]
Therefore, the overall rate constant is
k = k₂k₁/k-1
