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

For answer, constant example 3.12, on Nernst equation.
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise N.C.E.R.T. EXERCISE|18 Videos

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise Short Answer Type Questions|22 Videos

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise Example|74 Videos

  • D-AND -F BLOCK ELEMENTS

    DINESH PUBLICATION|Exercise BRAIN STORMING MULTIPLE CHOICE QUESTIONS (MCQS)|13 Videos

  • ETHERS

    DINESH PUBLICATION|Exercise (MCQs)|8 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.