Balance the following oxidation-reduction occurring in acidic solution. MnO₄^-(aq)+ Cr²⁺(aq)$\to$Mn²⁺(aq)+ Cr³⁺(aq) A) MnO₄^-(aq)+ 8H⁺(aq)+ 5Cr²⁺(aq)$\to$ Mn²⁺(aq)+ 4H₂O( $\ell$ )+ 5Cr³⁺(aq) B) MnO₄^-(aq)+ 8H⁺(aq)+ Cr²⁺(aq)$\to$Mn²⁺(aq)+ 4H₂O( $\ell$ )+ Cr³⁺(aq) C) MnO₄^-(aq)+ 4H₂(g)+ 5Cr²⁺(aq)$\to$ Mn²⁺(aq)+ 4H₂O( $\ell$ )+ 5Cr³⁺(aq) D) MnO₄^-(aq)+ 8H⁺(aq)+ 2Cr²⁺(aq)$\to$ Mn²⁺(aq)+ 4H₂O( $\ell$ ) + 2Cr³⁺(aq) E) MnO₄^-(aq)+ Cr²⁺(aq)$\to$Mn²⁺(aq)+ 2O₂(g)+ Cr³⁺(aq)

Question

Quizplus · Accepted Answer

The balanced equation is:
MnO4- + 8H+ + 5Cr2+ → Mn2+ + 4H2O + 5Cr3+
To balance the reduction half-reactions:
Cr2+ → Cr3+
2e-
To balance the oxidation half-reactions:
MnO4- → Mn2+
8H+ + MnO4- + 5e- → Mn2+ + 4H2O
Multiply reduction half-reaction by 5 and add to oxidation half-reaction:
MnO4- + 8H+ + 5Cr2+ → Mn2+ + 4H2O + 5Cr3+

Balance the Following Oxidation-Reduction Occurring in Acidic Solution →\to→ Mn2+(aq)+ Cr3+(aq) A) MnO4-(aq)+ 8H+(aq)+ 5Cr2+(aq)

Balance the Following Oxidation-Reduction Occurring in Acidic Solution $\to$ Mn²⁺(aq)+ Cr³⁺(aq)
A) MnO₄^-(aq)+ 8H⁺(aq)+ 5Cr²⁺(aq)