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Consult the table of standard electrode ...

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

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`Fe^(2+)rarr Fe^(3+)+e^(-),` `E^(c-)``_(o x i d)=-0.77V`
Only those substances can oxidize `Fe^(2+)` to `Fe^(3+)` whiCHM are stonger oxidizing agents than `0.77V` so that the `EMF` of the cell reaction is positive. This is so for elements lying below `Fe^(3+)|Fe^(2+)` in the electroCHMemical series, `e.g., Br_(2), Cl_(2), ` and `F_(2)`
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Consult the table of standard electrode potential and suggest three substances that can oxidize Fe^(2+) ions under suitable conditions.

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Assertion:Lithium has the lowest electrode potential. Reason: Lithium ion is the strongest oxidising agent.

(i) On the basis of the standard electrode potential values stated for acid solutions, predict whether Ti^(4+) species may be used to oxidise Fe(II) to Fe(III) {:(Ti^(4+) + e^(-) to Ti^(3+), E^(@) = +0.01V), (Fe^(3+) + e^(-) to Fe^(2+), E^(@)= +0.77V):} (ii) Based on the data arrange Fe^(3+), Mn^(2+) " and " Cr^(2+) in the increasing order of stability of +2 oxidation state. (Give a brief reason) E_(Cr^(3+)//Cr^(2+))^(@) = -0.4V E_(Mn^(3+)//Mn^(2+))^(@) = +1.5V E_(Fe^(3+)//Fe^(2+))^(@) = +0.8V

Value of standard electrode potential for the oxidation of Cl^(-) ions is more positive than that of water, even then in the electrolysis of aqueous sodium chloride, why is Cl^(-) oxidsied at anode instead of water?

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 reactions is not correct ?

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 couples will have highest value of emf ?

The standard reduction potential at 298 K for single electrodes are given below.l From this we can tell that

Using the standard electrode potentials given in Table, predict if the reaction between the following is feasible : Fe^(3+)(aq) and I^(c-)(aq)

Using the standard electrode potentials given in the Table 8.2, predict if the reaction between the following is feasible: Ag^(+)(aq) and Cu(s)

CENGAGE CHEMISTRY ENGLISH-NCERT BASED EXERCISE-Nuclear Chemistry (NCERT Exercise)
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