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`.

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 .

Consider the following redox reaction Mg_((S)) +Sn_((aq))^(2+) rarr Mg_((aq))^(2+)+Sn_((s)) : Write the cell formula.

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

Identify the type of reaction Na_2SO_(4(aq))+BaCl_(2(aq))rarrBaSO_(4(s))+2NaCl_((aq))

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.

Write Nernst Equation for the following reactions:- Cr(s) + 3Fe^(3+)(aq) rarrCr^(3+)(aq) + 3Fe^(2+)(aq)

Consider the following redox reaction Mg_((s))+Sn_(aq)^(2+) rarr Mg^2+ Sn_((s)) Calculate E_(cell) for the reaction at 25^@C if [Mg^(2+)] = 0.035M, [Sn^(2+)] = 0.025M , E_(Mg)^0 =- 2.37V and E_(Sn)^0 =-0.136V .

The following redox reaction occursin a galvanic cell. 2AI_((s))+3Fe_((aq))^(2+)(1M)rarr 2AI_((aq))^(3+)(1M)+3Fe : Write the cell notation.