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Chapter 19: Problem 17

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.

Short Answer

Expert verified
The species with the more positive reduction potential in each pair is the better oxidizing agent. The exact answers would depend on the values obtained from a standard reduction potentials table. However, as a general rule of thumb, elements in their elemental state, such as \( \mathrm{Br}_{2}\) and \( \mathrm{H}_{2}\), have a reduction potential of zero. Thus, unless the other species in the pair has a negative standard reduction potential, they are usually the weaker oxidizing agents. Additionally, \( \mathrm{O}_{2}\) in acidic media is generally a stronger oxidizing agent compared to \( \mathrm{O}_{2}\) in basic media.

Step by step solution

01

- Identify Reduction Potentials

Use a standard reduction potentials table to find the reduction potential for each species in the pairs. Using this data, the better oxidizing agent can be determined because the one with the greater standard reduction potential is a better oxidizing agent.
02

- Compare Reduction Potentials

Compare the reduction potentials of \( \mathrm{Br}_{2}\) and \( \mathrm{Au}^{3+}\). The species with the more positive reduction potential is the better oxidizing agent. Do the same comparison for each pair.
03

- Identify Oxidizing Agents

Repeat step 2 for the remaining pairs \( \mathrm{H}_{2}\) and \( \mathrm{Ag}^{+}\), \( \mathrm{Cd}^{2+}\) and \( \mathrm{Cr}^{3+}\), and \( \mathrm{O}_{2}\) in acidic media and \( \mathrm{O}_{2}\) in basic media. This will complete the evaluation of the better oxidizing agent for each pair.

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Most popular questions from this chapter

A sample of iron ore weighing \(0.2792 \mathrm{~g}\) was dissolved in an excess of a dilute acid solution. All the iron was first converted to \(\mathrm{Fe}(\mathrm{II})\) ions. The solution then required \(23.30 \mathrm{~mL}\) of \(0.0194 \mathrm{M} \mathrm{KMnO}_{4}\) for oxidation to Fe(III) ions. Calculate the percent by mass of iron in the ore.

An aqueous solution of a platinum salt is electrolyzed at a current of 2.50 A for \(2.00 \mathrm{~h}\). As a result, \(9.09 \mathrm{~g}\) of metallic \(\mathrm{Pt}\) are formed at the cathode. Calculate the charge on the Pt ions in this solution.

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.

How does the tendency of iron to rust depend on the \(\mathrm{pH}\) of solution?

The passage of a current of 0.750 A for 25.0 min deposited \(0.369 \mathrm{~g}\) of copper from a \(\mathrm{CuSO}_{4}\) solution. From this information, calculate the molar mass of copper.
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