Problem 1
Sketch a graph with two curves showing Pressure vs. Volume for two different values of the number of moles of gas, with \(n_{2}>n_{1}\), both at the same temperature. Explain the comparison of the two curves.
Problem 2
Sketch a graph with two curves showing Pressure vs. \(1 /\) Volume for two different values of the number of moles of gas, with \(n_{2}>n_{1}\), both at the same temperature. Explain the comparison of the two curves.
Problem 3
Sketch a graph with two curves showing Volume vs. Temperature for two different values of the number of moles of gas, with \(n_{2}>n_{1}\), both at the same pressure. Explain the comparison of the two curves
Problem 4
Sketch a graph with two curves showing Volume vs Temperature for two different values of the pressure of the gas, with \(P_{2}>P_{1}\), both for the same number of moles. Explain the comparison of the two curves.
Problem 6
Amont on's Law says that the pressure of a gas is proportion al to the absolute temper ature for a fixed quantity of gas in a fixed volume. Thus, \(P=k(N, V) T\). Demonstrate that Amonton's Law can be derived by combining Boyle's Law and Charles' Law.
Problem 7
Using Boyle's Law in your reasoning, demonstrate that the "constant" in Charles' Law, i.e. \(k_{2}(N, P),\) is inversely proportional to \(P\).
Problem 9
Using Dalton's Law and the Ideal Gas Law, show that the partial pressure of a component of a gas mixture can be calculated from $$P_{i}=P X_{i}$$ Where \(P\) is the total pressure of the gas mixture and \(X_{i}\) is the mole fraction of component \(i\), defined by $$ X_{i}=\frac{n_{i}}{n_{\text {total }}} $$
Problem 10
Dry air is \(78.084 \%\) nitrogen, \(20.946 \%\) oxygen, \(0.934 \%\) argon, and \(0.033 \%\) carbon dioxide. Determine the mole fractions and partial pressures of the components of dry air at standard pressure.
