Galvanic cell Is a device which converts chemical energy to electrical energy.Give the diagrammatic representation of the cell `Mg//MgSO_4 II CuSO_4//Cu`. Write the half-cell reactions take place in this cell.

Galvanic cell Is a device which converts chemical energy to electrical energy.Explain the mechanism of corrosion using electro chemical theory.

Galvanic cell Is a device which converts chemical energy to electrical energy.How many coulombs of electricity are required for the reduction of 1mol of MnO_4^- to Mn^(2+) ?

Diagrammatlcally represent H_2-O_2 fuel celland write thehalf ceil reactions taking place in this cell.

What is the energy transformation that takes place in a solar cell?

The chemical reactions taking place in electro chemical cells are redox reactions. In a Daniel cell , c) Write the chemical equation of the reaction taking place at anode.

One of the fuel cell uses the reaction of hydrogen and oxygen to form water. Write down the cell reaction taking place in the anode and cathode of the fuel cell.

Fuel cells are galvanic cells in which the chemical energy of fuel is directly converted into electrical energy. Type of fuel cell is a hydrogen - oxygen fuel cell. It consists of two electrodes made up of two porous graphite impregnated with a catalyst (platinum, silver, or metal oxide). The electrodes are placed in aqueous solution of NaOH. Oxygen nad hydrogen are continuously fed into the cell. Hydrogen gets oxidized to H^(oplus) which is neutralized by overset(Θ)(OH) , ie., anodic reaction. H_(2) hArr 2H^(oplus) + 2e^(-) 2H^(oplus) + 2 overset(Θ)(OH) hArr 2H_(2)O H_(2) + 2 overset(Θ)(OH) hArr 2H_(2)O + 2e^(-) At cathode, O_(2) gets reduced to overset(Θ)(OH) i.e., O_(2) + 2H_(2)O + 4e^(-) hArr overset(Θ)(4)OH Hence, the net reaction is 2H_(2) + O_(2) hArr 2H_(2)O The overall reaction has Delta H= -285.6kJ mol^(-1) and Delta G= -237.4kJ mol^(-1) " at " 25^(@)C Suppose the concentration of hydroxide ion in the cell is doubled, then the cell voltage will be

Fuel cells are galvanic cells in which the chemical energy of fuel is directly converted into electrical energy. Type of fuel cell is a hydrogen - oxygen fuel cell. It consists of two electrodes made up of two porous graphite impregnated with a catalyst (platinum, silver, or metal oxide). The electrodes are placed in aqueous solution of NaOH. Oxygen and hydrogen are continuously fed into the cell. Hydrogen gets oxidized to H^(oplus) which is neutralized by overset(Θ)(OH) , ie., anodic reaction. H_(2) hArr 2H^(oplus) + 2e^(-) 2H^(oplus) + 2 overset(Θ)(OH) hArr 2H_(2)O H_(2) + 2 overset(Θ)(OH) hArr 2H_(2)O + 2e^(-) At cathode, O_(2) gets reduced to overset(Θ)(OH) i.e., O_(2) + 2H_(2)O + 4e^(-) hArr overset(Θ)(4)OH Hence, the net reaction is 2H_(2) + O_(2) hArr 2H_(2)O The overall reaction has Delta H= -285.6kJ mol^(-1) and Delta G= -237.4kJ mol^(-1) " at " 25^(@)C If the cell voltage is 1.23V for the H_(2)-O_(2) fuel cell and for the half cell: O_(2) + 2H_(2) O + 4e^(-) hArr 4 overset(Θ)(OH) " has " E^(Θ) = 0.40V , then E^(Θ) " for " 2H_(2)O + 2e^(-) hArr H_(2) + 2 overset(Θ)(OH) will be