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Byju's Answer
Standard XII
Chemistry
Effect of Catalyst
The energy of...
Question
The energy of activation for Ist order reaction is 104.5 kJ
m
o
l
−
1
and pre-exponential factor A in Arrhenius equation is
5
×
10
13
s
e
c
−
1
. The temperature at which reaction have half-life of 1 minute in K is __________.
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Solution
k
=
0.693
t
1
/
2
=
0.693
60
......(1)
k
=
A
e
−
E
a
/
R
T
=
5
×
10
13
×
e
−
104500
8.314
T
......(2)
From (1) and (2)
0.693
60
=
5
×
10
13
×
e
−
104500
8.314
T
2.31
×
10
−
16
=
e
−
104500
8.314
T
=
e
−
12569.2
T
l
n
(
2.31
×
10
−
16
)
=
−
12569.2
T
−
36
=
−
12569.2
T
T
=
349
K
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Similar questions
Q.
The energy of activation of a first order reaction is 104.5 kJ
m
o
l
−
1
and pre-exponential factor (A) is
5
×
10
13
s
e
c
−
1
. At what temperature, will the reaction have a half life of 1 minute?
Q.
The energy of activation of a first order reaction is 104.5 kJ
m
o
l
e
−
1
and pre-exponential factor (A) is
5
×
10
13
s
e
c
−
1
.
At what temperature, will be reaction have a half life of 1 minute in kelvin?
Q.
In Arrhenius equation for a certain reaction, the values of
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13
s
e
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−
1
and
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m
o
l
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respectively. If the reaction is of first order, at what temperature will its half life period be
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Q.
In Arrhenius eauation for a certain reaction, the values of A and
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10
13
s
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and 98.6 kJ
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1
respectively. If the reaction is of first order, at what temperature will its half life period be 10 minutes ?
Q.
In Arrhenius equation for a certain reaction, the values of
A
and
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a
(activation energy) are
4
×
10
13
s
e
c
−
1
and
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m
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respectively. At what temperature, the reaction will have specific rate constant
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