Chapter 11

A balloon contains \(0.128 \mathrm{~mol}\) of gas and has a volume of \(2.76 \mathrm{~L}\). If an additional \(0.073 \mathrm{~mol}\) of gas is added to the balloon, what is its final volume? (Hint: The final number of moles is the sum of the initial number and the amount added.)

A sample of gas with an initial volume of \(28.4 \mathrm{~L}\) at a pressure of \(725 \mathrm{~mm} \mathrm{Hg}\) and a temperature of \(305 \mathrm{~K}\) is compressed to a volume of \(14.8 \mathrm{~L}\) and warmed to a temperature of \(375 \mathrm{~K}\). What is the final pressure of the gas?

A cylinder with a moveable piston contains \(218 \mathrm{~mL}\) of nitrogen gas at a pressure of \(1.32\) atm and a temperature of \(298 \mathrm{~K}\). What must the final volume be for the pressure of the gas to be \(1.55 \mathrm{~atm}\) at a temperature of \(335 \mathrm{~K}\) ?

A scuba diver takes a 2.8-L balloon from the surface, where the pressure is \(1.0 \mathrm{~atm}\) and the temperature is \(34^{\circ} \mathrm{C}\), to a depth of \(25 \mathrm{~m}\), where the pressure is \(3.5 \mathrm{~atm}\) and the temperature is \(18^{\circ} \mathrm{C}\). What is the volume of the balloon at this depth?

The total pressure in a \(11.7-\) Lautomobile tire is 44 psi at \(11^{\circ} \mathrm{C}\). How much does the pressure in the tire rise if its temperature increases to \(37{ }^{\circ} \mathrm{C}\) and the volume remains at \(11.7 \mathrm{~L}\) ?

What is the pressure in a 20.0-L cylinder filled with \(0.683\) mol of nitrogen gas at \(325 \mathrm{~K}\) ?

A cylinder contains \(28.5 \mathrm{~L}\) of oxygen gas at a pressure of \(1.8 \mathrm{~atm}\) and a temperature of \(298 \mathrm{~K}\). How many moles of gas are in the cylinder?

A cylinder contains \(11.8 \mathrm{~L}\) of air at a total pressure of \(43.2\) psi and a temperature of \(25^{\circ} \mathrm{C}\). How many moles of gas does the cylinder contain? (Hint: You must convert each quantity into the correct units \((\mathrm{L}, \mathrm{atm}, \mathrm{mol}\), and \(\mathrm{K})\) before substituting into the ideal gas law.)

What is the pressure in millimeters of mercury of \(0.0115\) mol of helium gas with a volume of \(214 \mathrm{~mL}\) at \(45^{\circ} \mathrm{C}\) ? (Hint: You must convert each quantity into the correct units (L, \(\mathrm{atm}\), \(\mathrm{mol}\), and \(\mathrm{K}\) ) before substituting into the ideal gas law.)

How many moles of gas must be forced into a \(3.5\)-L ball to give it a gauge pressure of \(9.4\) psi at \(25^{\circ} \mathrm{C}\) ? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is \(14.7\) psi so that the total pressure in the ball is \(24.1 \mathrm{psi}\).