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

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 .

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

Balance the following chemical equations: Mg(OH)_(2(s))+HCl_((aq))rarrH_(2)O_((l))+MgCl_(2(aq))

The following redox reaction occurs in a galvanic cell. 2Al_((s))+3Fe_((aq))^(2+)(1M)rarr 2Al_((aq))^(3+)(1M)+3Fe : If E^@anode = -1.66 V and E^@cathode =-0.44 Calculate DeltaG^@ for reaction.

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 .

Formulate a cell for each of the following reactions:- Mg(s) + Br_2(l)rarr Mg^(2+)(aq),+ 2Br^-(aq)

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.

Formulate a cell from the following electrode reactions Au^(3o+) (aq) + 3e^(o-)rarrAu(s) Mg(s)rarr Mg^(2o+) (aq) + 2e^(o-)

For the following redox reactions, find the correct statement. Sn^(2o+) + 2F^(3o+) rarr Sn^(4o+) + 2Fe^(2o+)

The reaction, 2Br_((aq))^((-))+Sn_((aq))^2 rarr Br_(2(I)) +Sn_((s)) with the standard potentials, E_(Sn)^@ = -0.114V, E_(Br_2)^@ = +1.09V , is