Caculate the `E_(cell)^@` for the following reaction at 298K:
`2Cr(s)+3Fe^(2+)(0.01M)rarr2Cr^(3+)(0.01M)+3Fe(s)`
Given `E_(cell)=0.261V`.

Calculate the e.m.f of the following cell at 298K 2Cr(s)+3Fe^(2+)(0.01M)rarr2Cr^(3+)(0.1M)+3Fe(s) Given: E^@(Cr^(3+)|Cr)=-0.75V , E^@(Fe^(2+)|Fe)=-0.45V .

Write the Nernst equation and calculate E.M.F of the following reaction at 298 K Mg // Mg^(2+) (0.1 M)"//" Cu^(2+) (0.01 M) // Cu (s) given E_("cell")^0 = 2.71V,F=96500 C//mol

calculate the e.m.f of the cell in which the following reaction takes place: Ni(s) +2Ag^(+) (0.002M)rarrNi^(2+) (0.160 M)+2Ag(s) Given that E_(cell)^o=1.05V

Calculate the emf of the following cell at 298k : Feabs(Fe^(2+)(0.001M)) abs(H^+(1M)) H_2(g)(1 b a r ),Pt(s) (given E^@,_(cell)=+0.44V )

Write Nernst equation for the following cell reaction: 2Al(s)+3Fe^(2+)(aq)rarr2Al^(3+)(aq)+3Fe(s)

Write NERNST equation also Calculate the cell e.m.f. and DeltaG for the cell reaction at 25^(@)C Cr(s)//Cr^(3+)(0.1M)"//"Fe^(2+)(0.01M)//Fe(s) Given E_(Cr^(3+)//Cr)^(0)=-0.75V, E_(Fe^(2+)//Fe)^(0)=-0.45V

Calculate the e.m.f. of the following cell at 298 K. Mg_((s))|Mg^(2+)(0.001M)||Cu^(2+)(0.0001M)|Cu_((s)) Given E^(@)(Cu^(2+)|Cu)=0.34V and E^(@)(Mg^(+)|Mg)=-2.37V .

Calculate the emf of the cell in which the following reaction takes place: Ni(s) + 2Ag^+ (0.002 M) Ni^(2+) (0.160 M) + 2Ag(s) Given that E^V_(cell) = 1.05 V

Calculate the potential of the following cell reaction at 298K: Sn^(4+)(1.50M)+Zn(s)rarrSn^(2+)(0.5M)+zn^(2+)(2.0M) The standard potential of the cell is 0.89V, will the potential of the cell will increase or decrease if the concentration of Sn^(2+) is increased in the cell?