Prove that T755=2T505 for first order reaction
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Explanation:
For a first order reaction, we have
t=
t
2.303
log
[A]
[A]
0
Let a M be the initial concentration.
When reaction is 99% complete,
[A]=a−
100
99a
=0.01a
t
99
=
k
2.303
log
0.01a
a
t
99
=
k
2.303
×2 ......(1)
When reaction is 90% complete,
[A]=a−
100
90a
=0.1a
t
90
=
k
2.303
log
0.1a
a
t
90
=
k
2.303
×1 ......(2)
Divide equation (1) by (2), we get
t
90
t
99
=2 ⟹t
99
=2t
90
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