Advertisements
Advertisements
Question
Using the standard electrode potential, predict if the reaction between the following is feasible:
Br2(aq) and \[\ce{Fe^{2+}_{( aq)}}\]
Advertisements
Solution
A reaction is feasible if the value of \[\ce{E^{\circ}_{cell}}\] is positive.
The reaction is as follows:
\[\ce{Fe^{2+}_{( aq)} + 1/2Br2_{( aq)} -> Fe^{3+}_{( aq)} + Br^-_{( aq)}}\]
According to this, the cell will be as follows:
\[\ce{Fe^{2+}_{( aq)} | Fe^{3+}_{( aq)} || 1/2Br2_{( aq)} | Br^-_{( aq)}}\]
∴ \[\ce{E^{\circ}_{cell} = E^{\circ}_{\frac{1}{2} Br_2/Br^-} - E^{\circ}_{Fe^{3+}/Fe^{2+}}}\]
= 1.09 − 0.77
= 0.32 V
Since the value of \[\ce{E^{\circ}_{cell}}\] is positive, hence the reaction is feasible.
APPEARS IN
RELATED QUESTIONS
Predict the product of electrolysis in the following:
An aqueous solution of 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:
A dilute solution of H2SO4 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 potential, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{I^-_{ (aq)}}\]
Using the standard electrode potential, predict if the reaction between the following is feasible:
\[\ce{Ag^+_{ (aq)}}\] and Cu(s)
Using the standard electrode potential, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{( aq)}}\] and \[\ce{Br^-_{( aq)}}\]
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?
