We are being asked to balance the given oxidation-reduction reaction. The reaction is under acidic conditions. When balancing redox reactions under acidic conditions, we will follow the following steps.
Step 1: Separate the whole reaction into two half-reactions
Step 2: Balance the non-hydrogen and non-oxygen elements first
Step 3: Balance oxygen by adding H2O to the side that needs oxygen (1 O: 1 H2O)
Step 4: Balance hydrogen by adding H+ to the side that needs hydrogen (1 H: 1 H+)
Balance the following reaction under acidic conditions.
Cr2O2−7(aq) + Fe2+(aq) → Cr3+(aq) + Fe3+(aq)
A. 7H2O(l) + Cr2O2−7(aq) + Fe2+(aq) → 2Cr3+(aq) + Fe3+(aq) + 14OH−
B. 14H+ + Cr2O2−7(aq) + Fe2+(aq) → 2Cr3+(aq) + Fe3+(aq) + 7H2O(l)
C. 7H2O(l) + Cr2O2−7(aq) + 6Fe2+(aq) → 2Cr3+(aq) + 6Fe3+(aq) + 14OH−
D. 14H+ + Cr2O2−7(aq) + 6Fe2+(aq) → 2Cr3+(aq) + 6Fe3+(aq) + 7H2O(l)
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