Question

at which of the following conditions concentration cell formed by hydrogen electrode will work spontaneously if concentration of hydrogen ions are C1 and C2 respectively



if answered correctly then I will post a question of 100 marks ​

Answer 1

Explanation:

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

i hope my answer is correct