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Chapter 19: Problem 13

Predict whether \(\mathrm{Fe}^{3+}\) can oxidize \(\mathrm{I}^{-}\) to \(\mathrm{I}_{2}\) under standard-state conditions.

Short Answer

Expert verified
Yes, \(Fe^{3+}\) can oxidize \(I^{-}\) to \(I_{2}\) under standard-state conditions due to the higher reduction potential of the half reaction \(Fe^{3+} + e^- \rightarrow Fe^{2+}\) compared to the half reaction \(2I^{-} \rightarrow I_{2} + 2e^-\).

Step by step solution

01

Identify the Half Reactions

Recognize that Fe3+ will be reduced to Fe2+ and I- will be oxidized to I2. So we have the following half-reactions: \(Fe^{3+} + e^- \rightarrow Fe^{2+}\) and \(2I^{-} \rightarrow I_{2} + 2e^-\)
02

Determine the Half-Cell Potentials

We can look up the standard electrode potentials for these half-reactions. From tables, we know that: E0(Fe3+/Fe2+) = +0.77 volts and E0(I2/2I-) = +0.54 volts.
03

Check for Spontaneity

Fe3+ has a higher reduction potential than I-. Therefore, Fe3+ will gain electrons, reducing to Fe2+, and I- will lose electrons, oxidizing to I2. The reaction is spontaneous under standard conditions as the reduction potential for the Fe3+/Fe2+ half-cell is greater than the I2/2I- half-cell.

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Most popular questions from this chapter

Which species in each pair is a better oxidizing agent under standard-state conditions? (a) \(\mathrm{Br}_{2}\) or \(\mathrm{Au}^{3+},\) (b) \(\mathrm{H}_{2}\) or \(\mathrm{Ag}^{+}\) (c) \(\mathrm{Cd}^{2+}\) or \(\mathrm{Cr}^{3+},\) (d) \(\mathrm{O}_{2}\) in acidic media or \(\mathrm{O}_{2}\) in basic media.

For a number of years it was not clear whether mercury(I) ions existed in solution as \(\mathrm{Hg}^{+}\) or as \(\mathrm{Hg}_{2}^{2+}\). To distinguish between these two possibilities, we could set up the following system: $$ \mathrm{Hg}(l) \mid \text { soln } \mathrm{A} \| \text { soln } \mathrm{B} \mid \mathrm{Hg}(l) $$ where soln A contained 0.263 g mercury(I) nitrate per liter and soln B contained 2.63 g mercury(I) nitrate per liter. If the measured emf of such a cell is \(0.0289 \mathrm{~V}\) at \(18^{\circ} \mathrm{C},\) what can you deduce about the nature of the mercury(I) ions?

Which species in each pair is a better reducing agent under standard-state conditions? (a) \(\mathrm{Na}\) or \(\mathrm{Li},\) (b) \(\mathrm{H}_{2}\) or \(\mathrm{I}_{2},\) (c) \(\mathrm{Fe}^{2+}\) or \(\mathrm{Ag}\), (d) \(\mathrm{Br}^{-}\) or \(\mathrm{Co}^{2+}\).

The hydrogen-oxygen fuel cell is described in Section 19.6 . (a) What volume of \(\mathrm{H}_{2}(g)\), stored at \(25^{\circ} \mathrm{C}\) at a pressure of 155 atm, would be needed to run an electric motor drawing a current of \(8.5 \mathrm{~A}\) for \(3.0 \mathrm{~h} ?\) (b) What volume (liters) of air at \(25^{\circ} \mathrm{C}\) and \(1.00 \mathrm{~atm}\) will have to pass into the cell per minute to run the motor? Assume that air is 20 percent \(\mathrm{O}_{2}\) by volume and that all the \(\mathrm{O}_{2}\) is consumed in the cell. The other components of air do not affect the fuel-cell reactions. Assume ideal gas behavior.

Write the Nernst equation and explain all the terms.
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