Free Redox Reactions and Electrochemistry Quiz | University Admission Chemistry Practice

Redox Reactions and Electrochemistry

Question 1 of 5

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The apparatus shows the titration of acidified iron(II) solution with potassium manganate(VII). The ionic equation is \[ \mathrm{MnO_4^-(aq) + 5Fe^{2+}(aq) + 8H^+(aq) \rightarrow Mn^{2+}(aq) + 5Fe^{3+}(aq) + 4H_2O(l)}. \]

Which statement is correct?

Select one option.

\([\mathrm{Fe^{2+}}] = 0.0160\ \text{mol dm}^{-3}\); \(\mathrm{Fe^{2+}}\) is the reducing agent; manganese changes from \(+7\) to \(+2\).
\([\mathrm{Fe^{2+}}] = 0.0800\ \text{mol dm}^{-3}\); \(\mathrm{MnO_4^-}\) is the reducing agent because it gives up oxygen.
\([\mathrm{Fe^{2+}}] = 0.00320\ \text{mol dm}^{-3}\); \(\mathrm{Fe^{2+}}\) is oxidised; manganese changes from \(+7\) to \(+2\).
\([\mathrm{Fe^{2+}}] = 0.0800\ \text{mol dm}^{-3}\); \(\mathrm{Fe^{2+}}\) is the reducing agent; manganese changes from \(+7\) to \(+4\).
\([\mathrm{Fe^{2+}}] = 0.0800\ \text{mol dm}^{-3}\); \(\mathrm{Fe^{2+}}\) is the reducing agent; manganese changes from \(+7\) to \(+2\).

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