Home
Class 12
CHEMISTRY
The half cell reactions with reduction p...

The half cell reactions with reduction potentials are
`Pb(s) to Pb^(+2) (aq), E_("red")^(@) =-0.13 V`
`Ag(s) to Ag^(+) (aq) , E_("rod")^(@) =+0.80 V`
Calculate its emf.

Text Solution

AI Generated Solution

To calculate the electromotive force (emf) of the cell given the half-cell reactions and their reduction potentials, follow these steps: ### Step 1: Identify the half-cell reactions and their reduction potentials. - For Lead (Pb): \( \text{Pb(s)} \rightarrow \text{Pb}^{2+}(aq) + 2e^- \) Reduction potential, \( E_{\text{red}} = -0.13 \, \text{V} \) - For Silver (Ag): ...
Promotional Banner

Topper's Solved these Questions

  • REDOX REACTIONS

    AAKASH INSTITUTE ENGLISH|Exercise Try Yourself|28 Videos

  • REDOX REACTIONS

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (Section A) (Objective type Questions (one option is correct))|40 Videos

  • PRINCIPLES OF QUALITATIVE ANALYSIS

    AAKASH INSTITUTE ENGLISH|Exercise Assignment (SECTION H)|9 Videos

  • SOLUTIONS

    AAKASH INSTITUTE ENGLISH|Exercise ASSIGMENT (SECTION-J) AAKASH CHALLENGERS QUESTIONS|10 Videos

Similar Questions

Explore conceptually related problems

At 20^(@) C, the standard oxidation potential of Zn and Ag in water are: Zn(s)rarr Zn^(2+) (aq) + 2e^(-), E^(o) = 0.76V , Ag(s) rarr Ag^(+)(aq) + E^(-) , E^(o) = - 0.80 V The standard EMF of the given reaction is: Zn+2Ag^(+)rarr 2AG+Zn^(+2)

Calculate the reduction potential for the following half cell reaction at 298 K. Ag^(+)(aq)+e^(-)toAg(s) "Given that" [Ag^(+)]=0.1 M and E^(@)=+0.80 V

The standard oxidation potential of Zn and Ag in water at 20^(@) C" are: " Zn(s) rarr Azn^(2+) (aq) + 2e^(-) E^(o) = 0.76 V Ag(s) rarr Ag^(+)(aq) +e^(-) E^(o) = - 0.80 V Which one of the following reactions actually takes place?

Standard reduction potential of the half cell reactions are given below Co^(3+)(aq) + e^(1-) to Co^(2+)(aq) , E^0 = +1.81 V Au^(3+)(aq) + 3e^(1-) to Au(s) , E^0 = +1.40 V I_(2)(s) + 2e^(1-) to 2I^(-)(aq) , E^0 = +0.54 V Cu^(2+)(aq) + 2e^(1-) to Cu(s) , E^0 = +0.34 V The strongest oxidizing and reducing agents respectively are:

A button cell used in watched funcations as follwing Zn(s)+Ag_(2)O(s)+H_(2)O(l)hArr2Ag(s)+Zn^(2+)(aq.)+2OH^(-)(aq) If half cell potentials are Zn^(2+)(aq.)+2e^(-) rarr Zn(s), E^(@) = -0.76 V Ag_(2)O(s)+H_(2)O(l)+2e^(-) rarr 2Ag(s)+2OH^(-)(aq.),, E^(@) = 0.34V The cell potential will be

Consider the cell : Zn|Zn^(2+)(aq)(1.0M)||Cu^(2+)(aq)(1.0M)||Cu Thee standard reduction potentials are 0.350V for Cu^(2+)(aq)+2e^(-)rarrCu and -0.763V for Zn^(2+)(aq)+2e^(-) rarr Zn a. Write the cell reaction. b. Calculate the EMF of the cell. c. Is the reaction spontaneous or not ?

Consider the following cell reaction Zn +2Ag^(o+)rarr Zn ^(2+)+2Ag. Given that E^(c-)._(Zn^(2+)(aq)Zn(s))=-0.76V E^(c-)._(Ag^(o+)(aq)Ag(s))=0.80V a. Calculate the standard EMF fo the cell. b. Which ion is more powerful oxidizing agent ? c. Which metal is more powerful reducing agent ?

Consider the following cell reaction Zn +2Ag^(o+)rarr Zn ^(2+)+2Ag. Given that E^(c-)._(Zn^(2+)(aq)Zn(s))=-0.76V E^(c-)._(Ag^(o+)(aq)Ag(s))=0.80V a. Calculate the standard EMF fo the cell. b. Which ion is more powerful oxidizing agent ? c. Which metal is more powerful reducing agent ?

Standard oxidation potential for the following half-cell reactions are [Fe(s) rarr Fe^(2+)(aq) + 2e^(-) E^3 = +0.44 V] [Co(s)rarr Co^(3+) (aq) + 3e^(-) E^0 = - 1.81 V The standard emf of the cell reaction [3Fe(s) +2Co^(3+) (aq)rarr 3Fe^(2+) (aq) + 2Co(s)] , will be

For the cell Zn((s)) |ZN^(2+) ((aq)) || M^(X+)((aq))|M((s)) , different half cells and their standard electrode potentials are given below : If E_(ZN^(2+)|ZN^(@))= -0.76V , which cathode will give a maximum value of E_(cell)^(@) per electron transferred ?