Two aqueous species undergo redox chemistry in acidic solution according to the…
CHEMISTRY · Multi-part · A Level · Chemistry · Oxidation, reduction and redox reactions · Oxidation, reduction and redox reactions
Problem
Two aqueous species undergo redox chemistry in acidic solution according to the half-reactions shown below. Coefficients may or may not be correct.
Half-reaction 1 (acidic): Cr2O72−+14H++6e−→2Cr3++7H2O
Half-reaction 2 (acidic): NO2−+H2O→NO3−+2H++2e−
(a) Verify that each half-reaction is individually balanced for both mass and charge under acidic conditions. Clearly show all corrections necessary to achieve balance.
(b) Combine the two balanced half-reactions to write the overall balanced ionic equation for the reaction occurring in acidic medium. Use the smallest set of whole-number coefficients.
(c) In the overall reaction you obtained in part (b), identify the oxidizing agent and the reducing agent, and state the total number of electrons transferred per formula unit of each reagent consumed.