Home
Class 12
CHEMISTRY
The cell in which the following reaction...

The cell in which the following reaction occurs, `2Fe^(3+) (aq) + 2I^(-)(aq) rarr 2Fe^(2+) (aq) + I_(2)(s)`
has `E_("cell")^(@) = 0.236V` at 298K , calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Text Solution

Verified by Experts

Two half reactions for the given redox reaction may be written as`:`
`2Fe^(3+) (aq) + 2e^(-) rarr 2Fe^(2+) ( aq)`
`2I^(-) rarr I_(2) + 2e^(-)`
2 moles of electrons are involved in the reaction, so n =2.
`Delta_( r ) G^(@) = -n FE_("cell")^(@)`
`= -( 2 "mol") xx( 96500 C "mol"^(-1)) xx ( -.236 V ) `
`= - 45548 CV = - 45548J`
`Delta _(r )G^(@) = - 45.55kJ`
`log K_(C ) = - ( Delta G^(@))/( 2.303 R T )`
`= - ( ( - 45.55kJ ))/( 2.303 xx ( 8.314 xx 10^(-3)kJ K^(-1)) xx ( 298 K))`
= 7.983
`K_( C ) =` antilog ( 7.983) `= 9.616 xx 10^(7)`
`K_( C ) = 9.616 xx 10^(7)`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise QUESTIONS FOR PRACTICE ( PART III ELECTROLCHEMICAL CELLS AND SERIES , NERNST EQUATIONS, BATTERIES AND CORROSION ) ( LONG ANSWER TYPE QUESTIONS) |3 Videos

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise QUESTIONS FOR ASSESSMENT ( PART III ELECTROLCHEMICAL CELLS AND SERIES , NERNST EQUATIONS, BATTERIES AND CORROSION ) ( MULTIPLE CHOICE TYPE QUESTIONS) |2 Videos

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise QUESTIONS FOR PRACTICE ( PART III ELECTROLCHEMICAL CELLS AND SERIES , NERNST EQUATIONS, BATTERIES AND CORROSION ) ( SHORT ANSWER TYPE I QUESTIONS) |14 Videos

  • D-BLOCK ELEMENTS

    ARIHANT PUBLICATION|Exercise Chapter practice (Long answer type questions)|2 Videos

  • ELEMENTS : NITROGEN FAMILY

    ARIHANT PUBLICATION|Exercise CHAPTER PRACTICE ( Long Answer Type Questions ) |11 Videos

Similar Questions

Explore conceptually related problems

Represent the galvanic cell in which the reaction, Zn(s) + Cu^(2+) (aq) rarr Zn^(2+) (aq) + Cu(s) take place.

The reaction, Cu^(2+)(aq) +2CI^- (aq) rarr Cu(s) +CI_2(g) has E_(cell)^@=1.03V .This reaction :

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

Calculate the standard cell potential of a galvanic cell in which the following reaction takes place 2Cr(s) + 3Cd^(2+) ( aq) rarr 2Cr^(3+) ( aq) + 3Cd(s) Calculate Delta_( r) G^(@) and equilibrium constant K of the above reaction at 25^(@)C . [Given, E_(Cr^(3+) //Cr)^(@) = - 0.74 V, E_(Cd^(2+)//Cd)^(@) = - 0.40V, 1F = 96500 C "mol"^(-1)]

Formulate the galvanic cell in which the following reaction takes place. Zn (s) + 2Ag^(+) ( aq) rarr Zn^(2+) (aq) + 2Ag(s) (i) Which one of its electrodes is negatively charged ? (ii) The reaction taking place at each of its electrode. (iii) The carriers of current within this cell.

Consider the following cell reaction, 2Fe(s) + O_(2)(g) + 4H^(+)(aq) rarr 2Fe^(2+) ( aq) + 2H_(2) O ( l ) , E^(@) = 1.67 V At [ Fe^(2+) ] = 10^(-3) M, p ( O_(2)) = 0.1 atm and pH =3. What is the cell potential at 25^(@)C ?

Derive Nerst equation for EMF of the following cell. Zn (s) + Cu^2+ (aq) rarr Zn^2+ (aq) + Cu(s)

Co(s) +Cu^(2+)(aq) rarrCo^(2+)(aq) +Cu(s) .This reaction is :