For the cell :
`Cr(s)|Cr^(3+)||Fe^(2+)|Fe(s)`
`DeltaG^(@)=-nFE^(@)`, the value of n will be :

Cr(s)| Cr^(3+)||Fe^(2+)|Fe(s) In the above cell, the value of n in the Nernst equation i.e., E=E^(@) - (0.059)/(n) log_(10)Q will be :

Cr(s)| Cr^(3+)||Fe^(2+)|Fe(s) In the above cell, the value of n in the Nernst equation i.e., E=E^(@) - (0.059)/(n) log_(10)Q will be :

Find out work done for the given cell Cr| Cr^(+3)|| Fe^(+2)| Fe E_(Cr//Cr^(2+))^(@) = 0.74V, E_(Fe^(2+)//Fe)^(@) = -0.44V

For the galvantic cell Pt(s)|Fe^(2+),Fe^(3+)"||"Fe^(2+)"|"Fe cell reaction is

What is the potential for the cell Cr|Cr^(3+)(0.1M)||Fe^(2+)(0.01M)|Fe E^(@)Cr^(3+)// Cr=-0.74V , E^(@)Fe^(2+)//Fe=-0.44V

The EMF of the cell, Cr|Cr^(+3) (0.1M) ||Fe^(+2) (0.01M)|Fe (Given: E^(0) Cr^(+3)|Cr =- 0.75 V, E^(0) Fe^(+2)|Fe =- 0.45 V)

What is the potential for the cell Cr|Cr^(3+)(0.1M)||Fe^(2+)(0.01M)|Fe E^(@)Cr^(3+)// Cr=-0.74V , E^(@)Fe^(2+)//Fe=-0.44V