Home
Class 12
CHEMISTRY
Calculate the e.m.f. of the cell in whic...

Calculate the e.m.f. of the cell in which the following reaction takes place :
`Ni(s) +2Ag^(+)(0.002 M)to Ni^(2+)(0.160 M)+2Ag(s)`
Given `E_(cell)^(@)`=1.05 v

Text Solution

Verified by Experts

`E_(cell)=E_(cell)^(@)-(0.0591)/(n)log[(Ni^(+2))]/([Ag^(+)]^(2)`
`=1.05 -(0.0561)/(2)log(0.160)/(0.002^(2)`
`=1.05-(0.0591)/(2)xx4.6`
=1.05-0.14=0.91 V
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE|Exercise Try Yourself|19 Videos

  • ELECTROCHEMISTRY

    AAKASH INSTITUTE|Exercise Assignment (SECTION A) Objective Type Questions (One option is correct)|43 Videos

  • COORDINATION COMPOUNDS

    AAKASH INSTITUTE|Exercise Assignment (Section-J Aakash Challenger Questions )|10 Videos

  • ENVIRONMENTAL CHEMISTRY

    AAKASH INSTITUTE|Exercise ASSIGNMENT (SECTION-D) (Assertion - Reason Type Questions)|5 Videos

Similar Questions

Explore conceptually related problems

Calculate the EMF of the cell in whiCHM the following reaction takes place : Ni(s)+2Ag^(o+)(0.002M) rarr Ni^(2+)(0.160M)+2Ag(s)

Calculate the emf of the cell in which the following reaction takes place Ni(s) + 2Ag_((0.002M))^(+) rarr Ni_((0.160M))^(2+) + 2Ag_((s)) Given E_("Cell")^(@) = 1.07V

Represent the cell in which following reaction takes place : Mg(s)+2Ag^(o+)(0.0001M)rarr Mg^(2+)(0.130M)+2Ag(s) calculate its E_(cell) if E^(c-)._(cell)=3.17V.

Calculate the e.m.f. of the cell in which the redox reaction is : Mg(s)+2Ag+(aq) to Mg^(2+)(aq)+2Ag(s) when [Mg^(2+)]=0.130 M and [Ag^(+)]=1.0xx10^(-4) M . Given E_(Mg^(2+)//Mg)^(@)=-2.37 V and E_(Ag^(+)//Ag)^(@)=+0.80 V .

Calculate emf of the following cell reaction at 2968 K : Ni(s)//Ni^(2+)(0.01 M) || Cu^(2+)(0.1 M)//Cu(s) [Given E_(Ni^(2+)//Ni)^(@)=-0.25" V ",E_(Cu^(2+)//Cu)^(@)=+0.34 " V " ] Write the overall cell reaction.