Calculate `E_(cell)^@, DeltaG^@` and equilibrium constant for the reaction : `2Cu_((aq))^+ rarr Cu_((aq))^(2+)+ Cu_((s))` `E_(Cu+//Cu)^@=0.52V and E_(Cu+/Cu)^@=0.16V`

Calculate equilibrium constant for the reaction, Ni_((s)) + 2Ag_((aq))^(2+) rarr Ni_((aq))^(2+) + 2Ag_((s)) at 25^@C E_(Ni)^@ =- 0.25V and E_(Ag)^@ = 0.799V .

Calculate standard Gibbs energy change and equilibrium constant at 25^@C for the cell reaction, Cd (s) + Sn^(2o+) (aq) rarr Cd^(2o+) (aq) + Sn (s) Given : E_(Cd)^@ = -0.403V and E_(Sn)^@ = -0.136 V . Write formula of the cell.

How are DeltaG^@, E^@(cell) and equilibrium constant related for a particular reaction?

Calculate the equilibrium constant for the redox reaction at 25^@C , Sr_((s))+Mg_((aq))^2+ rarr Sr_((aq))^(2+) Mg_((s)) that occursina galvaniccell. Write thecell formula. E_(Mg)^@ = - 2.37 V and E_(Sr)^@ = -2.89 V .

The standard potential for the cell reaction 2Ti_((S)) + Hg^(2+) (1M) rarr 2Ti^+ (1 M) + Hg_((I)) Where E_(Ti)^@ =- 0.34V, E_(Hg)^@ = 0.86 V is

Write the expression for the equilibrium constant, K_C for each of the following reactions: 2Cu(NO_3)_2 hArr 2CuO(s) + 4 NO_2(g)

What is standard cell potential for the reaction 3Ni (s) + 2Al^(3+)(1M)rarr3Ni^(2o+)(1M) + 2Al(s) if E_(Ni)^0 =- 0.25 V and E_(AI)^0 = -1.66V ?

Calculate the standard cell potentials of galvanic cell in which the following reactions take place 2Cr_((s)) + 3Cd_((aq))^(2+)rarr 2Cr_(aq)^(3+) + 3Cd E_(Cr)^@ = -0.740 V, E_(Cd)^@ = -0.403 V, Calculate the Delta_rG^@ and equilibrium constant of the reactions.

What is standard cell potential for the reaction Cell notation 3Ni(s) + 2AI^(3o+) (1M) rarr 3Ni^(2o+) (1M) + 1Al(s) if E_(Ni)^@ =-0.25 V and E_(AI)^0 =-1.66V?

Write the Nernst equation and emf of the following cells at 298K. Mg_((s))| Mg_(aq)^(2+)(0.001M)| Cu_((s)) (Given E_(Mg^(2+)//Mg)^@ = -2.37 V, E_(Cu^(2+) //Cu)^@=0.34V)