Home
Class 12
CHEMISTRY
Calculate the electrical work (at standa...

Calculate the electrical work (at standard state) obtained from galvanic cell : `Mg|Mg^(2+)(aq)||Ag^(+)(aq)|Ag`
Given : `E_(Mg^(2+)|Mg)^(@)=-2.36V and E_(Ag^(2+)|Ag)^(@)=+0.80V`

Text Solution

Verified by Experts

`{:("Anode reaction: "Mg(s)" "rarr" "Mg^(2+)(aq)+2e),("Cathode reaction : "2Ag^(+)(aq)+2e" "rarr" "2Ag(s)),(bar(" Cell reaction: "Mg(s)+2Ag^(2+)(aq)" "rarr" "Mg^(2+)(aq)+2Ag(s))):}`
As 2 mol electrons are involved in the cell reaction, n = 2.
The standard EMF of the cell, `E_("cell")^(@)=E_("cathode")^(@)-E_("anode")^(@)`
`=E_(Ag^(+)|Ag)^(@)-E_(Mg^(2+)|Mg)^(@)=0.80-(-2.36)=+3.16V`
Therefore, the electrical work doen by the cell,
`W_("el")=nFE_("cell")^(@)`
`2xx96500xx3.16=609880" V.C"=609.88kJ.`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    CHHAYA PUBLICATION|Exercise PROBLEM|7 Videos

  • ELECTROCHEMISTRY

    CHHAYA PUBLICATION|Exercise WARM UP EXERCISE|62 Videos

  • D - AND F - BLOCK ELEMENTS

    CHHAYA PUBLICATION|Exercise PRACTICE SET 8 (Answer the following questions)|10 Videos

  • ENVIRONMENTAL CHEMISTRY

    CHHAYA PUBLICATION|Exercise PRACTICE SET 14(Answer the following questions)|6 Videos

Similar Questions

Explore conceptually related problems

Write cell reaction and calculate electrical work obtained from the following galvanic cell at standard condition . Mg|Mg^(2+)(aq)||Ag^(+)(aq)|Ag [Given : E_(Mg^(2+)|Mg)^(0) = -2.36 volt and E_(Ag^(+)|Ag)^(0) = 0.80 volt.]

Write cell reaction and calculate electrical work obtained from the following galvanic cell at standard condition: Mg|Mg^(2+)(aq)||Ag^+(aq)Ag . Given: E_(mg2+/mg)^@=-2.36 volt & E_(ag+/Ag)^@=0.80 Volt]

Calculate E_("cell")^(@) of the cell Mg|Mg^(2+)||Cu^(+)|Cu Given : E_(Mg^(2+)|Mg)^(@)=-2.37V and E_(Cu^(+)|Cu)^(@)=+0.15V .

It the reaction, 2Ag(s)+Fe^(2+)(aq)rarr2Ag^(+)(aq)+Fe(s) possible? Given : E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Ag^(+)|Ag)^(@)=+0.80V .

For the given cell, Mg|Mg^(2+)||Cu^(2+)|Cu -

Determine DeltaG^(@) and the value of the equilibrium constant for the following reaction occurring in an electrochemical cell at 25^(@)C . Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s) Given that, E_(Cu^(2+)|Cu)^(@)=0.34V and E_(Ag^(+)|Ag)^(@)=0.80V

For the galvanic cell, Cu|Cu^(2+)(0.13M)||Ag^(+)(0.01M)|Ag (ii) Is the cell reaction spontaneous ? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Ag^(+)|Ag)^(@)=+0.80V] .

Write down the appropriate Nernst equation for the following voltaic cell and calculate the e.m.f. of the cell at 298 K. Fe(s)|Fe^(2+)(0.002M)||Ag^(+)(0.02M)|Ag(s) ["Given, "E_(Fe^(2+)|Fe)^(@)=-0.44V and E_(Ag^(+)|Ag)^(@)=+0.80V" at 298K"]

What will be the standard electrode potential for the change, Fe^(3+)(aq)+e rarr Fe^(2+)(aq). Given : E_(Fe^(3+)|Fe)^(@)=-0.036V, E_(Fe^(2+)|Fe)^(@)=-0.439V

Calculate the E.M.F. for the cell given below Mg(S)|Mg^(2+)(0.001)(M)||Cu^(2+)(0.01M)|Cu(S) given E_(Mg^(2+)//Mg)^@ =-2.36V. E_(Cu^(2+)//Mg)^@ =+0.34V