The cell in which the following cell reaction occurs,
`2Fe _((aq))^(3+)+2I_((aq))^(-)to 2Fe _((aq))^(2+)+I_(2(s))`
has `E_(cell)^(0)=0.236V` at 298 K. Calculate the standard Gibbs energy and the equilibrium costant of the cell reaction.

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

Calculate the standard cell potentials of galvanic cell in which the following reactions take place. (i) 2Cr(s) + 3Cd^(2+)(aq) to 2Cr^(3+) (aq) + 3Cd (ii) Fe^(2+)(aq) + Ag^(+)(aq) to Fe^(3+)(aq) + Ag(s) Calculate the ΔrG and equilibrium constant of the reactions.

Fe_((aq))^(+3)+SCN_((aq))^(-) harr [Fe(SCN)]_(aq)^(+2) is an example of

Calculate the equilibrium constant of the reaction : Cu_((s))+2Ag_((aq))^(+)to Cu_((aq))^(2+)+2Ag_((a)) E_((cell))^(Θ)=0.46V

The equilibrium constant of the reaction Cu_((s)) + 2Ag_((aq))^(+) iff Cu_((aq))^(+2) + 2Ag_((s)) , " is " x xx 10^(15) , 'x' is ( E^(@) = 0.46 V at 298 K )

Write the cell reaction taking plce in the cell CU_((s))|Cu_((aq))^(+2)||Ag _((aq))^(+) |Ag _((s))

The emf of the cell in which of the following reaction , Zn_((s)) +Ni^(2+) (0.1 M) to Zn^(2+) (1.0M) + Ni_((s)) occurs is found to 0.5105 V at 298 K . The standard emf of the cell is