Home
Class 12
CHEMISTRY
Consider the following reaction, Zn(s)...

Consider the following reaction,
`Zn(s)+Cu^(2+) (0.1 M) rarr Zn^(2+) (1 M)+Cu(s)` above reaction, taking place in a cell, `E_("cell")^(@)` is `1.10 V. E_("cell")` for the cell will be `(2.303 (RT)/(F)=0.0591)`

A

2.14 volt

B

1.80 volt

C

1.07 volt

D

0.82 volt

Text Solution

Verified by Experts

The correct Answer is:
C
`E=E^(@)-(0.059)/(n)"log"([Zn^(++)])/([Cu^(++)])=1.10-(0.059)/(2)"log"(1)/(0.1)`
`=1.10-0.0295log10=1.07` volt
Promotional Banner

Similar Questions

Explore conceptually related problems

For the redox reaction: Zn(s) +Cu^(2+) (0.1M) rarr Zn^(2+) (1M)+Cu(s) taking place in a cell, E_(cell)^(@) is 1.10 volt. E_(cell) for the cell will be (2.303 (RT)/(F) = 0l.0591)

For the redox change , Zn_(s) + underset (0.1M)FuCu^2+ rarr underset(Zn^(2+))(1M) + Cu_((s)) , Taking place in a cell E_(cell)^@ is 1.10 volt . E_(cell) for the cell would be :

Consider the following reaction, Cu|Cu^(2+) (1M)||(Zn^(2+)(1 M)|Zn A cell represented above should have emf

Consider the following cell reaction Cu(s)+2Ag^(+)(aq) rarr Cu^(2+) (aq) +2Ag(s) E_("cell")^(@)=0.46 V By boubling the concentration of Cu^(2+) , E_("cell") is

What is the Gibbs energy of the following reaction? Zn(s)+Cu^(2+) (aq) rarr Zn^(2+)(aq)+Cu^(2+) (s), E_("cell")^(@)=1.1 V