Chemistry

Chemistry

Problem

In acidic solution, Fe2+\text{Fe}^{2+} reacts with MnO4−\text{MnO}_4^- according to the unbalanced equation below. MnO4−+Fe2+→Mn2++Fe3+\text{MnO}_4^-+\text{Fe}^{2+}\rightarrow\text{Mn}^{2+}+\text{Fe}^{3+} After the equation is completely balanced using the lowest whole-number coefficients, what is the coefficient for Fe2+\text{Fe}^{2+}? a) 1010 b) 77 c) 55 d) 33
Intuitive explanation

This is a redox reaction where you need to track electron transfer between species. Identify what's being oxidized (Fe2+\text{Fe}^{2+} loses electrons) and what's being reduced (MnO4−\text{MnO}_4^- gains electrons), then use the half-reaction method to balance electrons lost and gained. Once the electrons match, combine the half-reactions and simplify to lowest whole-number coefficients.

Intuitive explanation

This is a redox reaction where you need to track electron transfer between species. Identify what's being oxidized (Fe2+\text{Fe}^{2+} loses electrons) and what's being reduced (MnO4−\text{MnO}_4^- gains electrons), then use the half-reaction method to balance electrons lost and gained. Once the electrons match, combine the half-reactions and simplify to lowest whole-number coefficients.

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