Home
Class 12
CHEMISTRY
Represent the cell in which following re...

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. `

Text Solution

Verified by Experts

The cell reaction in terms of cell notation is
`Mg|Mg^(2+)(0.130 M)||Ag^(+)(0.001 M)|Ag`
`E_(cell)=E_(cell)^(@)-(0.0591)/(n)"log"([Anode])/([Cathode])`
`=(3.17)-(0.0591)/(2)"log"(0.130)/(0.0001)^(2)=(3.17)-(0.0591)/(2)"log"(0.0591)/(2)"log"(0.130)/(10^(-8))`
`=(3.17)-0.02955" log "(1.3xx10^(7))=(3.17)-(0.02955xx7.1139)`
`=(3.17-0.21)=2.69 V`.
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise IN-TEXT QUESTIONS|15 Videos

  • ELECTROCHEMISTRY

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

  • ELECTROCHEMISTRY

    DINESH PUBLICATION|Exercise ULTIMATE PREPARATORY PACKAGE|12 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

Represent the cell in which the following reaction takes place: Mg(s)+2Ag^(+)(0.0001M)toMg^(2+)(0.130M)+2Ag(s) Calculate its E_(cell) . Given that E_(Mg^(2+)//Mg)^(@)=-2.37V and E_(Ag^(+)//Ag)^(@)=+0.80V

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)

Knowledge Check

  • Calculate emf of the cell in which the following reaction takes place :- Ni_(s) + 2Ag^(+) (0.002M) to Ni^(+2) (0.160M) + 2Ag_((s)) Given : E_("cell")^(o) = 1.05V, (2.303RT)/(F) = 0.06, log2 = 0.3

    A
    `1.05 V`
    B
    `0.912 V`
    C
    `1.19 V`
    D
    `2.05 V`

  • An unknown mtal, M, and its salt, M(NO_(3)_(2) are combined with a half-cell in which the following reaction occurs: 2Ag^(+) + M rightarrow 2Ag + M^(2+) Ag^(+)(aq) + e(-) rightarrow Ag(s) [E_(red)^(@) = 0.80V] If E_(cell)^(@) = 1.36V, what is E_(red)^(@) for M^(2+)(aq) + 2e^(-) rightarrow M(s) ?

    A
    0.56V
    B
    0.24V
    C
    `-0.24V`
    D
    `-0.56V`

    • Similar Questions

    Explore conceptually related problems

    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

    Calculate the emf of the cell in which the following reaction takes place: Ni(s)+2Ag^(+)(0.002M)toNi^(2+)(0.160M)+2Ag(s) Given that E_(cell)^(@)=1.05V

    Calculate the emf 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 that: E_("cell")^(@) = 1.05 V

    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

    Calculate emf of the following cell at 298 K : Mg(s)+2Ag^(+)(0.0001M)rarrMg^(2+)(0.130M)+2Ag(s) ["Given : "E_("cell")^(theta)=3.17V]

    The following chemical reaction is occurring in an electrochemical cell Mg (s) + 2Ag^(+) (0.0001 M) to Mg^(2+) (0.10 M) + 2Ag (s) The E° electrode values are Mg^(2+)//Mg = - 2.36 V, Ag^(+)//Ag = 0.81 V For lids cell calculate/write (a) (i) E° value for the electrode 2Ag^(+)//2Ag (ii) Standard cell potential E_("cell")^(@) (b) Cell potential E_("cell") , (c) (i) Symbolic representation of the above cell. (ii) Will the above cell reaction be spontaneous ?

    Home
    Profile