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Chapter 19: Problem 39

The compound \(\mathrm{Pb}_{3} \mathrm{O}_{4}\) (red lead) contains a mixture of lead(II) and lead(IV) oxidation states. What is the mole ratio of lead(II) to lead(IV) in \(\mathrm{Pb}_{3} \mathrm{O}_{4} ?\)

Short Answer

Expert verified
The mole ratio of lead(II) to lead(IV) in \(\mathrm{Pb}_{3} \mathrm{O}_{4}\) is 2:1.

Step by step solution

01

Determine the oxidation states of lead in the compound

To start, let's consider lead's oxidation states in the compound and identify the lead(II) and lead(IV) components. Since the total charge of a compound must be neutral, we can use this information to determine the oxidation states. The oxygen atoms in the compound have a total charge of 4 * (-2) = -8. For the lead atoms, let's use x, y, and z to represent the oxidation states of the three lead atoms, where x and y represent the lead(II) atoms and z is the lead(IV) atom. The sum of these oxidation states must balance the total charge of the oxygen atoms: 2x + z = +8
02

Solve for the oxidation states

Now, we will solve for the oxidation states: 2x + z = +8 Since x represents lead(II) atoms and y represents lead(IV) atoms, we know that x = +2 and z = +4. We can plug these values back into the equation above to solve for the number of lead(II) atoms: 2(+2) + (+4) = +8 4 + 4 = +8
03

Calculate the mole ratio of lead(II) to lead(IV)

Now that we know there are two lead(II) atoms and one lead(IV) atom in the compound, we can calculate the mole ratio by dividing the moles of lead(II) by the moles of lead(IV): Mole ratio of lead(II) to lead(IV) = moles of lead(II) / moles of lead(IV) Mole ratio of lead(II) to lead(IV) = 2/1 Thus, the mole ratio of lead(II) to lead(IV) in \(\mathrm{Pb}_{3} \mathrm{O}_{4}\) is 2:1.

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Most popular questions from this chapter

Write balanced equations describing the reaction of lithium metal with each of the following: \(\mathrm{O}_{2}, \mathrm{S}, \mathrm{Cl}_{2}, \mathrm{P}_{4}, \mathrm{H}_{2}, \mathrm{H}_{2} \mathrm{O},\) and HCl.

Draw Lewis structures for the \(\mathrm{AsCl}_{4}^{+}\) and \(\mathrm{AsCl}_{6}^{-}\) ions. What type of reaction (acid-base, oxidation- reduction, or the like) is the following?$$2 \mathrm{AsCl}_{5}(g) \longrightarrow \mathrm{AsCl}_{4} \mathrm{AsCl}_{6}(s)$$.

In each of the following pairs of substances, one is stable and known, and the other is unstable. For each pair, choose the stable substance, and explain why the other is unstable. a. \(\mathrm{NF}_{5}\) or \(\mathrm{PF}_{5}\) b. \(\mathrm{AsF}_{5}\) or \(\mathrm{AsI}_{5}\) c. \(\mathrm{NF}_{3}\) or \(\mathrm{NBr}_{3}\)

\(\mathrm{Al}_{2} \mathrm{O}_{3}\) is amphoteric. What does this mean?

For each of the following, write the Lewis structure(s), predict the molecular structure (including bond angles), and give the expected hybridization of the central atom. a. \(\mathrm{KrF}_{2}\) c. \(\mathrm{XeO}_{2} \mathrm{F}_{2}\) b. \(\mathrm{KrF}_{4}\) d. \(\mathrm{XeO}_{2} \mathrm{F}_{4}\)
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