When solid iron(II) oxalate dihydrate,

CHEMISTRY · Multi-part · A Level · Chemistry · Oxidation, reduction and redox reactions · Oxidation, reduction and redox reactions

Problem

When solid iron(II) oxalate dihydrate, FeC2O4⋅2H2O(s)\mathrm{FeC_{2}O_{4} \cdot 2H_{2}O(s)}, is dissolved in acidic aqueous potassium permanganate, the following unbalanced reaction occurs at 25 °C25\,\text{°C}: FeC2O4(aq)\mathrm{FeC_{2}O_{4}(aq)} + MnO4−(aq)\mathrm{MnO_{4}^{-}(aq)} → Fe3+(aq)\mathrm{Fe^{3+}(aq)} + CO2(g)\mathrm{CO_{2}(g)} + Mn2+(aq)\mathrm{Mn^{2+}(aq)} Water and hydrogen ions are also present in the reaction mixture. (a) Balance the reaction in acidic solution, using the smallest whole-number coefficients. (b) State the total number of electrons that are transferred per formula unit of FeC2O4⋅2H2O\mathrm{FeC_{2}O_{4} \cdot 2H_{2}O} that reacts. (c) A 0.350 g0.350\,\text{g} sample of FeC2O4⋅2H2O\mathrm{FeC_{2}O_{4} \cdot 2H_{2}O} is completely consumed under the conditions described. Calculate the number of moles of electrons that move through the reaction mixture.

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