Question

Calculate cell potential of zn/cu having 0.77 M solution of Znso4 and 0.5M solution not cuso4 at 300k using Nernst equation Ered of cu is 0.34v and Ered of Zn is-0.76v​

Answer 1

Answer:

Given Zn∣Zn

2+

(0.001M)∣∣Cu

2+

(0.1M)∣Cu

Overall cell reaction:

Zn⟶Zn

2+

+2e

−

Cu

2+

+2e

−

⟶Cu

Zn+Cu

2+

⟶Zn

2+

+Cu

E

cell

o

=standard reduction potential of cathode + standard oxidation potential of anode

E

cell

o

=0.34 to 0.76 V

E

cell

o

=1.1 V

K

C

=

[Cu

2+

]

[Zn

2+

]

=

10

−1

10

−3

=10

−2

EMF of the cell at any electrode concentration is:

E=E

o

−

n

0.059

log(K

C

)=1.1−

2

0.059

log(10

−2

)=1.1−

2

0.059

×(2)=1.1−0.059=1.041V