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Tardigrade
Question
Chemistry
Consider following two reactions A longrightarrow Product -(d[A]/d t)=k1[A]0 B longrightarrow Product -(d[B]/d t)=k2[B] k1 and k2 are expressed in terms of molarity ( mol L -1) and time ( s -1) as :
Q. Consider following two reactions
A
⟶
Product
−
d
t
d
[
A
]
=
k
1
[
A
]
0
B
⟶
Product
−
d
t
d
[
B
]
=
k
2
[
B
]
k
1
and
k
2
are expressed in terms of molarity
(
m
o
l
L
−
1
)
and time
(
s
−
1
)
a
s
:
1804
157
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A
s
−
1
,
M
s
−
1
L
−
1
B
M
s
−
1
,
M
s
−
1
C
s
−
1
,
M
−
1
s
−
1
D
M
s
−
1
,
s
−
1
Solution:
Unit of rate constant
k
=
Time
1
⋅
(
conc.
)
n
−
1
1
For
k
1
n
=
0
k
=
t
1
⋅
(
con
c
)
0
−
1
1
hence
conc
⋅
t
−
1
≡
M
⋅
sec
−
1
k
2
n
=
1
k
=
t
1
⋅
(
con
c
)
1
−
1
1
=
t
1
=
s
−
1