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AP EAPCET 04-Jul-2022 Shift 2 Paper
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Section:
Chemistry
© examsiri.com
Question :
145 of 160
Marks:
+1
,
-0
38.6
amperes of current is passed for 100 seconds through an aqueous
C
u
S
O
4
solution using platinum electrodes. The mass of copper consumed from the solution and volume of gas liberated at STP are respectively (molar mass of
C
u
=
63.54
g
m
o
l
−
1
).
6.37
g
,
0.448
L
0.63
g
,
0.224
L
1.27
g
,
0.224
L
4
g
.
‌
‌
0.448
L
Validate
Solution:
(c) Given, current,
I
=
38.6
A
, Time,
t
=
100
s
Cathode
Cu
2
+
(
a
q
)
+
2
e
⊖
→
Cu
(
s
)
Anode
2
O
H
(
a
q
)
→
H
2
O
(
l
)
+
‌
1
2
O
2
(
g
)
+
2
e
⊖
Using Faraday's Ist law,
W
‌
=
Z
I
t
,
‌
‌
(
Z
→
‌
electrochemical equivalént
‌
)
‌
=
‌
E
I
t
96500
=
‌
M
I
t
2
×
96500
‌
=
‌
63.5
×
38.6
×
100
2
×
96500
=
1.27
g
1.27
g
‌
Cu
is deposited.
Using Faraday's second law,
‌
W
Cu
E
Cu
=
‌
W
o
2
E
O
2
⇒
‌
1.27
63.5
=
‌
W
O
2
16
W
O
2
=
‌
1.27
×
16
635
=
0.32
g
Moles of
O
2
=
‌
0.32
32
=
0.01
‌
mol
Volume of
O
2
at
STP
=
0.01
×
22.4
=
0.224
L
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