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Byju's Answer
Standard XII
Chemistry
Activation Energy
Calculate the...
Question
Calculate the activation energy for a reaction of which rate constants becomes 4 times when temperature changes from
30
0
C
to
50
0
C
[R= 8.314
J
m
o
l
−
1
K
−
1
]
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Solution
l
n
k
′
k
=
E
a
R
×
[
T
′
−
T
T
T
′
]
T
=
30
o
C
=
30
+
273
K
=
303
K
T
′
=
50
o
C
=
50
+
273
K
=
323
K
l
n
k
′
k
=
E
a
R
×
[
T
′
−
T
T
T
′
]
l
n
4
k
k
=
E
a
8.314
J
/
m
o
l
/
K
×
[
323
−
303
303
×
323
]
1.386
=
2.46
×
10
−
5
×
E
a
E
a
=
56400
J
/
m
o
l
E
a
=
56.4
k
J
/
m
o
l
because
1
k
J
=
1000
J
Note: Since rate constant becomes 4 times,
k
′
=
4
k
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2
Similar questions
Q.
The rate of a reaction triples when temperature changes from
20
o
C
to
50
o
C
. Calculate energy of activation for the reaction
(
R
=
8.314
JK
−
1
mol
−
1
,
l
o
g
10
3
=
0.477
)
.
(Give your answer to the nearest integer value)
Q.
The rate constant for a first order reaction becomes six times when the temperature is raised from
350
K
to
400
K
. Calculate the activation energy for the reaction.
[
R
=
8.314
J
K
−
1
m
o
l
−
1
]
Q.
The rate of a reaction becomes four times when the temperature changes from
293
K
to
313
K
. Calculate the energy of activation
(
E
2
)
of the reaction assuming that it does not change with temperature.
[
R
=
8.314
J
/
K
m
o
l
−
1
,
log
4
=
0.6021
]
Q.
The rate constant of a first order reaction becomes
5
times when the temperature is raised from
350
K to
400
K. Calculate the activation energy for the reaction. (Gas reactant R
=
8.314
J
K
−
1
m
o
l
−
1
).
Q.
What is the activation energy for a reaction if its rate doubles when the temperature is raised from
20
0
C
to
35
0
C
? (R = 8.314 J
m
o
l
−
1
K
−
1
)
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