Write the Nernst equation and emf of the following cells at 298 K.`Mg_(s)// Mg^(2+) (0.001M) II Cu(2+)(0.001M)// Cu_(s), E^0cell = 2.71 V`.

Write the Nernst equation and emf of the following'cells at -298 ~K: i. Mg(s) I M_g^2 *(0.001 M) II Cu^2+(0.0001 M) ICu(s) ii, Fe(s) I Fe^2+(0.001 M) II H^+(1 M) I H_2(~g)(lbar) I^2 Pt(s)^* ii. Sn(s) I Sn^2+(0.050 M) IHH^+(0.020 M) IH(g)(1 'bar)IPt(s) iv. Pt(s) IBr_3(I) IBr(0.010 M) IIH^+(0.030 M) L+H_2(~g) (1 bar)IPt(s).

Write the Nernst equation and emf of the following cells at 298 K. Sn_(s)//Sn^(2+) (0.050M) II H^+ (0.02M)//H_2(g) (1 bar) 1 Pt(S), E^0 Sn^(2+)//Sn=-0.14 V .

Calculate the e.m.f of the following concentration cell at 298K, Zn(s)| Zn^(2+)(0.1) || Zn^(2+) (1.0)|Zn(s)

Calculate the reduction potentials for the following half cells: Cu|Cu^(2+)(0.2M), E_(Cu^(2+),Cu)^@=0.34V

Derive expression to calculate emf (reduction) of the following half cells at 25^@C Cu^(2+)|Cu(s)

Calculate the reduction potential for the following half cells at 25^@C Mg|Mg^(2+) (1 times 10^-4 M), E_(Mg,Mg^(2+))^@=+2.36V

Nernst equation describes the variation of electrode potential with concentration and temperature. Write cell reaction, overall reaction and calculate e.m.f at 25C^0 for the cell. Also write Nernst equation for the cell potential. Mg//Mg_(10^(-3)M)^(2+)// Ag_(0.1M)^(+) // Ag Given E_(Mg^(2+)//Mg)^0 = 2.37V E _(Ag^+//Mg)^0=0.8V .

What is the emf of the following cell Pt:H_(2)(1"atm")|H^(+)(0.1M)||Cl_(2)(1"atm")|Cl^(-)(0.01M) at 298K(E_(Cl_(2))^(@)|Cl^(-)=1.36V)D

Calculate the emf of the cell in which the following reaction takes place: Ni(s)+ 2Ag^+(0.002M) to Ni^2(0.160 M)+2Ag(s) . Given that E_(cell)^0=1.05V

Calculate the following: i) (2.3 xx 3.2)/(0.4) ii) (0.01 xx .001)/(.1 xx 0.01)