Set up the cell consisting of `H_((aq))^+ | H_(2(g)) and Pb_(aq)^(2+)| Pb((s)) electrodes. Calculate the emf at `24^@C` of the `[Pb^(2+)] = 0.1 M, [H^+] = 0.5 M` and hydrogen gas is at 2 atm pressure. `E_(Pb)^@ = -0.126 V`.

Construct a cell consisting of Ni^(2+) |Ni half cell and H^+|H_2 (g. latm) | Pt half cell: Calculate emf of the cell if [Ni^(2+)]=0.1M[H^+]=0.05M and E_(NI)^0=-0.257 .

Calculate the number of moles of hydrogen and gas present in 0.5 m^3 sample of hydrogen gas at a pressure of 101.325 Pa and at 27^@C .

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 .

Given the reaction : C_((s)) + H_(2)O_((l)) rarr CO_((g)) + H_(2(g)) . Calculate the volume of the gases produced at STP from 48.0 g of carbon.

DeltaG^@ for the reaction Ag_((aq))^+ +1/2H_(2(g)) rarr H_((aq))^+ + Ag_((s)) , where standard potential for silver half cell reaction is 0.8V, will be

The volume strength of 3.0 M H_(2)O_(2) solution is

Calculate the voltage of the cell, Sn (s)|Sn^(2o+) (0.02M) || Ag^(o+) (0.01M)|Ag (s) at 25^@C . E^@= -0.136 V, E_(Ag)^@= 0.800 V .

Consider a galvanic cell that uses the half reactions: 2H_((aq))^+ +2e^- rarr H_(2(g)) Mg_((aq)) +2e^-rarrMg_((a)) Write balanced equation for the cell reaction. Calculate E_(Cell)^@ and DeltaG^@ if concentrations are 1M each and P_(H2)=10 atm. E_(Mg)^@=-2.37V .