Which one of the following cell is an example of concentration cell with transference? A) Pt/H₂(g). HCL (0.01)/HCI (0.1), H, (g)/Pt
B) Pt/H₂(g).HCL (0.01)/L.P./HCI(0.1), H₂(g)/Pt
C) Pt/H, (g), HCL (0.1)/HCI (0.01), H, (g) / Pt
D) Pt/H, (g), HCL (0.01)/LP./HCI (0.01), H₂(g)/Pt
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Explanation:
Answer
Correct option is
A
0.20V
The half-cell reactions are,
At Anode:
2
1
H
2
(g)→H
+
(aq)+e
−
At Cathode:AgCl(s)+e
−
→Ag(s)+Cl
−
(aq)
Complete reaction:AgCl(s)+
2
1
H
2
(g)→Ag(s)+Cl
−
(aq)+H
+
(aq)
We know,
E
cell
0
=E
cathode
0
−E
anode
0
=(SRP)
cathode
−(SRP)
anode
We know standard hydrogen potential is assumed to be zero.
So,(SRP)
anode
=0
Let, (SRP)
cathode
=x
So,
E
cell
0
=x
Now we use the Nernst equation,
E
cell
=E
cell
0
−
nF
2.303RT
log(Q)
⟹E
cell
=E
cell
0
−0.06×log([Cl
−
][H
+
])
n=1;
0.92=x−
1
0.06
log(10
−6
×10
−6
)
⟹x=0.20V
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