Home
Class 12
CHEMISTRY
(a) The cell in which the following reac...

(a) The cell in which the following reactions occurs:
`2Fe^(3+)(aq)=2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s)`
has `E_(cell)^(@)=0.236V` at 298 K. Calculate the standard Gibbs energy of the cell reaction.
(Given: `1F=96,500" C "mol^(-1)`)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: `1F=96,500" C "mol^(-1)`)

Text Solution

AI Generated Solution

### Solution: **(a)** To calculate the standard Gibbs energy (ΔG°) of the cell reaction, we can use the formula: \[ \Delta G^\circ = -nFE^\circ_{\text{cell}} \] ...
Promotional Banner

Topper's Solved these Questions

  • XII BOARDS

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise SET-II|32 Videos

  • XII BOARDS

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise SET-III|31 Videos

  • SAMPLE PAPER 2019

    XII BOARD PREVIOUS YEAR PAPER ENGLISH|Exercise SECTION: D|1 Videos

Similar Questions

Explore conceptually related problems

The cell in which the following reaction occurs 2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(aq)+I_(2)(s) has E_(cell)^(0)=0.236V at 298 K. Calculate the standard gibbs energy and the equilibrium constant of the cell reaction.

The cell in which the following reaction occurs : 2Fe_(aq)^(3+) + 2I_(aq)^(-) to 2Fe_(aq)^(2+) + I_(2(s)) "has" E_("cell")^(o) = 0.236 V "at" 298 K The equilibrium constnat of the cell reaction is

For the cell reaction: 2Fe^(3+)(aq)+2l^(-)(aq)to2Fe^(2+)(aq)+l_(2)(aq) E_(cell)^(ɵ)=0.24V at 298K . The standard gibbs energy (triangle,G^(ɵ)) of the cell reaction is [Given that faraday constnat F=96500Cmol^(-1)]

For the cell reaction 2Fe^(3+)(aq) + 2l^(-1) (aq) to 2Fe^(2+) (aq) + I_2(aq) E_("cell")^(Theta) = 0.24 V at 298 K. The standard Gibbs energy (Delta_r G^Theta) of the cell reaction is [Given that Faraday constnat F = 96500 C mol^(-1) ]

The reaction Cu^(2+)(aq)+2Cl^(-)(aq) rarr Cu(s)+Cl_(2)(g) has E^(c-)._(cell)=-1.03V . This reaction

Calculate the DeltaG^(@) of the following reaction :- Fe^(+2)(aq)+Ag^(+)(aq)toFe^(+3)(aq)+Ag(s) E_(Ag^(+)//Ag)=0.8V" "E_(Fe^(+3)//Fe^(+2))^(0)=0.77V

Consider the following cell reaction. 2Fe(s)+O_(2)(g)+4H^(+)(aq)rarr2Fe^(2+)(aq)+2H_(2)O(l), E^(@)=1.67V At [Fe^(2+)]=10^(-3)M,P(O_(2))=0.1 atm and pH=3, the cell potential at 25^(@)C is

The standard electrode potential for Deniell cell is 1.1V . Calculate the standard Gibbs energy for the reaction. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq)+Cu(s)

Consider the following reaction at equilibrium 2Fe^(2+)(aq)+Cu^(2+)to2Fe^(3+)(aq)+Cu When the reaction comes to equilibrium, what is the cell voltage ?

The standard electrode potential for Daniel cell is 1.1V . Calculate the standard Gibbs energy of the reaction (In KJ/mol) Zn_((s))+Cu_((aq))^(2+)rarrZn_((aq))^(2+)+Cu_((s))