the rate constant of a reaction doubled by an increase in temperature 10°C to 20°C what is the activation energy of the reaction
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ANSWER
Let K
1
=K
then K
2
=2K
T
1
=30
0
C+273
=303K T
2
=40
0
+273
=313K
log(
K
1
K
2
)=
2.303R
E
a
[
T
1
T
2
T
2
−T
1
]
or,log(
K
2K
)=
2.303X8.3
E
a
[
313X303
313−303
]
E
a
=54571KJ/mol
=54.5KJ/mol
≈54.66KJ/mol
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