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Byju's Answer
Standard XII
Chemistry
Entropy
If C-C, C-H...
Question
If
C
−
C
,
C
−
H
a
n
d
C
=
O
bond energies in acetaldehyde are
377
,
421
a
n
d
720
k
J
m
o
l
−
1
respectively, calculate the wavelength of radiation (in nm) required to bring about the photochemical decomposition of acetaldehyde.
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Solution
E
=
h
v
=
h
c
w
a
v
e
l
e
n
g
t
h
Δ
E
d
e
c
o
m
p
=
B
E
C
−
C
=
377
k
J
m
o
l
−
1
=
6.26
×
10
−
19
J
/
m
o
l
e
c
u
l
e
∴
λ
=
6.626
×
10
−
34
×
3
×
10
8
6.26
×
10
−
19
=
317.5
n
m
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0
Similar questions
Q.
The recombination of methyl radicals has no activation barrier. The activation energy values for the first step in the thermal thermal decomposition of acetaldehyde given and
E
p
h
o
t
o
c
h
e
m
i
c
a
l
are
309.32
k
J
m
o
l
−
1
and
41.8
k
J
m
o
l
−
1
respectively.
Calculate the overall activation energy for the thermal decomposition of acetaldehyde.
Q.
The arrhenius (pre exponential) factors and activation energy values for steps
(
i
)
to
(
i
v
)
are
A
1
,
A
2
,
A
3
,
A
4
a
n
d
E
1
,
E
2
,
E
3
a
n
d
E
4
respectively.
Calculate the overall activation energy
E
t
h
e
r
m
a
l
for the thermal decomposition of acetaldehyde.
Write the expression for overall activation energy,
E
p
h
o
t
o
c
h
e
m
i
c
a
l
of photochemical decomposition of acetaldehyde.
Q.
In the photochemical decomposition of acetaldehyde, one photon of absorbed light decomposes one molecule of
C
H
3
C
H
O
into
∙
C
H
3
a
n
d
∙
C
H
O
. If
′
I
′
a
b
s
is the intensity of light absorbed in the reaction. Write the rate equation for this photochemical decomposition. (Note: the first step in the photochemical reaction is temperature independent)
Calculate
[
∙
C
H
3
]
a
n
d
d
[
C
O
]
d
t
assuming steps (ii) to (iv) given are same and
[
∙
C
H
3
]
,
[
∙
C
H
3
C
O
]
are under steady state.
Q.
How will you bring about following conversions:
(a) Methane to methanol.
(b) Ethane to ethanol (acetaldehyde).
(c) Methane to methanoic acid.
Q.
At
518
o
C
, the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of
363
T
o
r
r
, was
1.00
T
o
r
r
s
−
1
when
5
%
had reacted and
0.5
T
o
r
r
s
−
1
when
33
%
had reacted. The order of the reaction is:
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