What is the value of `E^(@)` cell in the following reaction?
`Cr|Cr^(3+) (0.1 M)||Fe^(2+) (0.01 M)|Fe`
Given, `E_(Cr^(3+)//Cr)^(@)=-0.74 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V`

Calculate the e.f.m of the cell Cr|Cr^(3+)(0.1M)||Fe^(2+)(0.01M)|Fe [given that E_(Cr^(3+)//Cr)^(@)=-0.75,E_(Fe^(2+)//Fe)^(@)=-0.45V]

Calculate the e.f.m of the cell Cr|Cr^(3+)(0.1M)||Fe^(2+)(0.01M)|Fe [given that E_(Cr^(3+)//Cr)^(@)=-0.75,E_(Fe^(2+)//Fe)^(@)=-0.45V]

Calculate the e.m.f. of the cell at 25^(@)C Cr|Cr^(3+)(0.1M)||Fe^(2+)(0.01M)|Fe Given E_((Cr^(2+)//Cr))^(@)=-0.75V,E_((Fe^(2+)//Fe))^(@)=-0.44

Calculate the emf for the given cell at 25^(@)C . Cr| Cr^(3+) ( 0.1M) || Fe^(2+) ( 0.01M) | F e [Given, E_(Cr^(3+)//Cr)^(@)= -0.74V, E_(Fe^(2+)//Fe)^(@) = -0.44V ]

Calculate the emf of the cell at 25^(@)C Cr|Cr^(3+)(0.1M)||Fe ^(2+)(0.01M) |Fe, given that E_(Cr^(3+)//Cr )^(0)=-0.74V and E_(Fe ^(2+)//Fe )^(0)=-0.44V

Write NERNST equation also Calculate the cell e.m.f. and DeltaG for the cell reaction at 25^(@)C Cr(s)//Cr^(3+)(0.1M)"//"Fe^(2+)(0.01M)//Fe(s) Given E_(Cr^(3+)//Cr)^(0)=-0.75V, E_(Fe^(2+)//Fe)^(0)=-0.45V