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

The following redox reaction occursin a galvanic cell. 2AI_((s))+3Fe_((aq))^(2+)(1M)rarr 2AI_((aq))^(3+)(1M)+3Fe : Identify anode and cathode

The following redox reaction occursin a galvanic cell. 2AI-((s))+3Fe_((aq))(2+)(1M)rarr 2AI_((aq))^(3+)(1M)+3Fe : Calculate E_(Call)^@ if E_(anode)^@=-1.66 V and E_(Sn)^@=-0.136V, E_(Ag)^@=0.799V, (0.8744V)]=-0.44V .

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.

The cell reaction of the galvanic cell Cu_((s))|Cu_((aq))^(2+)"||"Hg_((aq))^(2+)|Hg_((l)) is __________.

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

Consider the following cell Pb_((s))|Pb_((aq))^(2+)(0.5M)||Cu_((aq)^(+2) (0.001M)| E^@Pb = -0.126V E°Cu = +0.337V: Write the cell reaction.

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.

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 .

Balance the following redox reactions by ion- electron method: Cr_2O_7^(2-) (aq) + SO_2 (g) rarr Cr^(3+) (aq) + SO_4^(2-) (aq) (in acidic solution)

Balance the following redox reactions by ion- electron method: H_2O_2 (aq) + Fe^(2+) (aq) rarr Fe^(3+) (aq) + H_2O (l) (in acidic solution)