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Consult the table of the standard electr...

Consult the table of the standard electrode potentials and suggest three substances that can oxidize ferrous ions under suitable conditions.

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To determine three substances that can oxidize ferrous ions (Fe²⁺) to ferric ions (Fe³⁺), we need to consult the standard electrode potential values. The oxidation of ferrous ions can be represented by the half-reaction: \[ \text{Fe}^{2+} \rightarrow \text{Fe}^{3+} + e^- \] The standard reduction potential (E°) for this half-reaction is -0.77 V. To oxidize Fe²⁺, we need substances that have a higher standard reduction potential than -0.77 V, as they will act as stronger oxidizing agents. ### Step-by-Step Solution: ...
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Consult the table of standard eletrode potentials and suggest three substances that can oxidise ferrous ions under suitable conditions

Consult the table of standard electrode potential and suggest three substances that can oxidize Fe^(2+) ions under suitable conditions.

Knowledge Check

  • If the standard electrode potential of an electrode is greater than zero, then we can infer that its

    A
    reduced from is more stable compared to hydrogen gas.
    B
    oxidised from is more stable compared to hydrogen gas.
    C
    reduced and oxidised forms are equally stable.
    D
    reduced from is less stable than the hydrogen gas.

  • Which defines the standard reduction electrode potential of Zn^(2+) ions

    A
    `Zn^(2+) (aq) + 2 e^(-) to Zn(s) , [Zn^(2+)] = 1 M`
    B
    `Zn(g) to Zn^(2+) + 2e^(-) , [Zn^(2+)] = 1 M`
    C
    `Zn^(2+) (aq) to Zn(s) + 2e^(-) , [ Zn^(2+)] = 1 M`
    D
    `Zn^(2+) (g) + 2 e^(-) to Zn(s) - 2e^(-) , [Zn^(2+)] = 1 M`

  • Which reagent can produce salicylic acid from sodium phenoxide under suitable conditions?

    A
    `K_(2)Cr_(2)O_(7)//H^(+)`
    B
    `CHCl_(3)//KOH`
    C
    `CO_(2)//dil. HCl`
    D
    `C Cl_(4)//KOH`

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    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.

    The name of equation showing relation between electrode potential (E) standard electrode potential (E^(@)) and concentration of ions in solution is

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    The potential associated. with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any gås appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0:0 volt. The electrode potential value for each electrode process is a measure, of relative tendency of the active species in the process to remain in the oxidized / reduced form. A negative E^@ means that the redox couple is a stronger reducing agent than the H^(+)//H_2 couple. A positive E mears that the redox couple is a weaker reducing agent than. the H^(+)//H couple. The metal with greater positive value of standard reduction potentlal forms the oxide of greater thermal stability: Which of the following oxides will be themally most stable?

    The potential associated with each electrode is known as electrode potential. If the concentration of each species taking part in the electrode reaction is unity (if any appears in the electrode reaction, it is confined to 1 atmospheric pressure) and further the reaction is carried out at 298 K, then the potential of each electrode is said to the standard electrode potential. By convention, the standard electrode potential of hydrogen electrode is 0.0 volt. The electrode potential value for each electrode process is a measure of relative tendency of the active species in the process to remain in the oxidised/reduced form. A negative E^(@) means that the redox couple is a stronger reducing agent than the H^(+)//H_(2) couple. A positive E^(@) means that the redox couple is a weaker reducing agent than the H^(+)//H_(2) couple. The metal with greater positive value of standard reduction potential forms the oxide of greater thermal stability. Which of the following oxides will be thermally most stable ?

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