Problem 1
State the Law of Combining Volumes and provide an example of your own construction which demonstrat es this law.
Problem 2
Explain how the Law of Combining Volumes, combined with the Atomic-Molecular Theory, leads directly to Avogadro's Hypothesis that equal volumes of gas at equal temperatures and pressure contain equal numbers of particles.
Problem 3
Use Avogadro's Hypothesis to demonstrate that oxygen gas molecules cannot be monatomic.
Problem 4
The density of water vapor at room temperature and atmospheric pressure is \(0.737 \frac{g}{L}\). Compound A is \(80.0 \%\) carbon by mass, and \(20.0 \%\) hydrogen. Compound \(\mathrm{B}\) is \(83.3 \%\) carbon by mass and \(16.7 \%\) hydrogen. The density of gaseous Compound \(\mathrm{A}\) is \(1.227 \frac{g}{L}\), and the density of Compound B is \(2.948 \frac{g}{L}\). Show how these data can be used to determine the molar masses of Compounds A and B, assuming that water has molecular mass 18 .
Problem 6
Explain the utility of calculating the number of moles in a sample of a substance.
Problem 7
Explain how we can conclude that \(28 \mathrm{~g}\) of nitrogen gas \(\left(N_{2}\right)\) contains exactly as many molecules as \(32 \mathrm{~g}\) of oxygen gas \(\left(O_{2}\right),\) even though we cannot possibly count this number.
