(a)
Interpretation:
The standard cell potential of the HCO−3/CO2−3,H2 couple has to be predicted.
Concept introduction:
The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by ΔrG° whereas ΔrG depends on the reaction condition and extent of reaction.
(b)
Interpretation:
The standard potential for the cell reaction Na2CO3(aq)+H2O(l)→NaHCO3(aq)+NaOH(aq) has to be predicted.
Concept introduction:
Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.
(c)
Interpretation:
The Nernst equation for the cell has to be stated.
Concept introduction:
Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,
Ecell=Eοcell−RTvFlnQ
Where,
- Ecell is the electrode potential of the cell.
- Eοcell is the standard electrode potential of the cell.
- R is the gas constant.
- T is the temperature.
- v is the number of electrons.
- F is the Faraday’s constant.
- Q is the reaction quotient.
(d)
Interpretation:
The change in cell potential when the pH is changed to 7.0 at 298 K has to be stated.
Concept introduction:
Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. The expression for Nernst equation is,
Ecell=Eοcell−RTvFlnQ
Where,
- Ecell is the electrode potential of the cell.
- Eοcell is the standard electrode potential of the cell.
- R is the gas constant.
- T is the temperature.
- v is the number of electrons.
- F is the Faraday’s constant.
- Q is the reaction quotient.
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Atkins' Physical Chemistry
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