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Nernst equation halps us to understand t...

Nernst equation halps us to understand the effect of `"______"` on the electrode of the half-cell and `emf` of the voltiv cell

A

temperature

B

concentrations of solultes

C

parical pressures of gases

D

All of these

Text Solution

Verified by Experts

The correct Answer is:
D
Electrode potentials and cell potentials and cell potentials, like Gibbs-energy chages, depends on temperture and on the compo-sition of the reacion mixture, i.e., on the concentrations of solutes and the partial pressures of gases.
The Nernst equation is used to calculate electrode potentials and cell potentials for temperature, concentrations and parical pressures other than standard state values.
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Calculating the cell emf for Nonstandard condition : A galvanic cell is constructed at 298 K as follows. One half-cell consists of a chlorine gas electrode (i.e. Cl_(2)//Cl^(-) couple) with the partial pressure of Cl_(2) = 0.100 bar and C_(CI-) = 0.100 M . The other half-cell involves the MnO_(4)^(-)//Mn^(2+) couple in acidic solution with C_(MnO_(4)^(-)) = 0.100 M, C_(Mn^(2+)) = 0.100 M , and C_(H+) = 1.00 M . Apply the Nernst equation to datermine the cell potenital for this cell. Strategy: First datermine the overall cell reaction and then calculate the standard cell potential (E_("cell")^(@)) from the standard electrode potenital in Table 3.1. then use the Nernst equation to find the cell potential (E) under cited conditions.

Calculating the emf from standard potentials: A galvanic cell consists of an Al electrode in a 1.0M Al(NO_(3))_(3) solution and an Fe electrode in a 1.0M Fe(NO_(3))_(2) solution. Calculate the standard emf of this electrohemical cell at 25^(@)C . Also write the cell reaction. Strategy: From the table of standard electrode potentials, write the two reduction half reaction and standard electrode potentials for the cell. Change the direction of the half-cell reaction corresponding tol the smaller (or more negative) electrode potential. Multiply the when the half-reactions are added the electrons cancel. The sum of the half-reactions is the cell reaction. Add the electrode potentials to get the cell emf.

Knowledge Check

  • Nernst equation is useful in determining

    A
    EMF of a cell
    B
    Equilibrium constant
    C
    Spontaneity of a cll reaction
    D
    All of these

  • nernst equation gives the effect of _____and____on the EMF of a cell.

    A
    Concentration of electrolytic solutions
    B
    temperature
    C
    Both a& b
    D
    None

  • The electrode potential of oxidation half cell

    A
    is independent of concentration of the ions in the cell
    B
    decreases with decreased concentration of the ions in the cell
    C
    decreases with increased concentration of the ions in the cell
    D
    is independent of temperature