Advertisements
Advertisements
प्रश्न
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Ag_{(s)}}\] and \[\ce{Fe^{3+}_{( aq)}}\]
Advertisements
उत्तर
A reaction is possible if the value of `"E"_"cell"^Θ` is feasible.
The reaction is as follows –
\[\ce{Ag_{(s)} + Fe^{3+}_{( aq)} -> Ag^{+}_{( aq)} + Fe^{2+}_{( aq)}}\]
According to this the cell will be as follows –
\[\ce{Ag_{(s)} | Ag^{+}_{( aq)} || Fe^{3+}_{( aq)} | Fe^{2+}_{( aq)}}\]
∴ `"E"_("cell")^Θ = "E"_("Fe"^(3+)//"Fe"^(2+))^Θ - "E"_("Ag"^+//"Ag")^Θ`
= 0.77 − 0.80
= −0.03 V
Since the value of `"E"_"cell"^Θ` is negative, hence the reaction is not feasible.
APPEARS IN
संबंधित प्रश्न
Predict the product of electrolysis in the following:
An aqueous solution of \[\ce{AgNO3}\] with silver electrodes.
Predict the product of electrolysis in the following:
An aqueous solution of AgNO3 with platinum electrodes.
Predict the product of electrolysis in the following:
An aqueous solution of CuCl2 with platinum electrodes.
How much electricity is required in coulomb for the oxidation of 1 mol of H2O to O2?
How much electricity is required in coulomb for the oxidation of 1 mol of FeO to Fe2O3?
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{I^-_{ (aq)}}\]
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Ag^+_{ (aq)}}\] and Cu(s)
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{Br^-_{ (aq)}}\]
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Br2_{(aq)}}\] and \[\ce{Fe^{2+}_{( aq)}}\]
In the following reaction, identify X:
\[\ce{Cr2O^{2-}7 + X ->[H+] Cr^{3+} + H2O + Oxidized product of X}\]
Write the reaction occurring at anode and cathode and the products of electrolysis of aq KCl.
Four half-reactions, I to IV are shown below:
- \[\ce{2Cl^- -> Cl2 + 2e^-}\]
- \[\ce{4OH^- -> O2 + 2H2O + 2e^-}\]
- \[\ce{Na^+ + e^- -> Na}\]
- \[\ce{2H^+ + 2e^- -> H2}\]
Which two of these reactions are most likely to occur when concentrated brine is electrolysed?
