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Stronger the oxidizing agent, greater is...

Stronger the oxidizing agent, greater is the

A

Reduction potential

B

Oxidation potential

C

lonic nature

D

None of the above

Text Solution

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The correct Answer is:
A
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Determining the directiom of spontaneity from electrode pot Na^(+)(aq.) + e^(-) rarr Na(s) E^(@) = -2.71 V entials : Predict from Table 3.1, whether Pb^(2+)(aq.) can oxidize Al(s) or Cu(s) under standard conditions. Calculate E^(ɵ) for each reaction at 25^(@)C . Strategy: To predict whether a redox reaction is spontaneous, remember that an oxidizing agent can oxidize any reducing agent that lies below it in the table but can't oxidize one that lies above it. Alternatively, write the expected reaction. Find the oxidizing agents in the equations, one is on the left side and the other on the right side. Locate these oxidizing agents in a table of electrode potentials (the oxidizing agent is on the left side of the reduction half-reaction). The stronger oxidizing agent is the one involved in the half-reaction with the more positive standard electrode potential.

Knowledge Check

  • Stronger the oxidising agent, greater is the

    A
    reduction potential
    B
    oxidation potential
    C
    ionic behaviour
    D
    none of these.

  • Stronger the oxidising agent , greater is the :

    A
    Oxidation potential
    B
    Reduction potential
    C
    Ionic behaviour
    D
    None

  • Stronger is oxidising agent, more is

    A
    standard reduction potential of that species
    B
    the tendency to get it self oxidised
    C
    the tendency to lose electrons by that species
    D
    standard oxidation potential of that species

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