AP Chemistry

Gas Laws WS #1

1. In a study to see how closely gaseous ammonia obeys Boyle’s law, several volume measurements were made at various pressures, using 1.0 mol NH3 gas at a temperature of 0ºC. Using the results listed below, calculate the Boyle’s law constant for NH3 at the various pressures. Does this experiment support Boyle’s Law?

2. Suppose we have a 12.2-L sample containing 0.50 mol oxygen gas (O2) at a pressure of 1 atm and a temperature of 25ºC. If all this O2 were converted to ozone (O3) at the same temperature and pressure, what would be the volume of the ozone? 3. A sample of diborane gas (B2H6), a substance that bursts into flame when exposed to air, has a pressure of 345 torr at a temperature of -15ºC and a volume of 3.48 L. If conditions are changed so that the temperature is 36ºC and the pressure is 468 torr, what will be the volume of the sample? 4. A deep underground cavern contains 2.24 x 106 L of methane gas (CH4) at a pressure of 2.40 atm. and a temperature of 42.0oC. How many kilograms of methane does this gas deposit hold? 5. A can of Lysol is designed to withstand internal pressures of up to 4.500 atm. How hot must the can get before it explodes, assuming that it has a volume of 0.400 L and an initial pressure of 3.00 atm at a temperature of 25.7ºC? 6. Three 1.00 L flasks at 25.0 °C and 1.00 atm pressure contain: CH4 (flask A), CO2 (flask B) and NH3 (flask C). Which flask (or none) contains 0.041 mol of gas? 7. You have just volunteered to decorate the gym for the winter dance with 300.0 Helium balloons. There is a store in town that will rent a 25 L. helium tank with a pressure of 30.0 atm. Each balloon, when filled, holds 2.5 L of helium gas at a pressure of 1.04 atm. Will one tank be enough to fill all 300.0 balloons? Assume that the gas temperature does not change as the balloons are filled. If not, how many balloons can be filled with the tank of gas? 8. A sample of nitrogen gas has a volume of 1.75 L at STP. How many moles of N2 are present? 9. What is height (in mm) of a column of ethanol if the pressure at the base of the column is 1.50 atm? (The density of Hg is 13.534 g/cm3 and ethanol is 0.789 g/cm3.) 10. An elemental gas has a mass of 10.3 g. If the volume is 58.4 L and the pressure is 758 torr at a temperature of 2.5 o C, what is the gas? 11. Quicklime (CaO) is produced by the thermal decomposition of calcium carbonate (CaCO3). Calculate the volume of CO2 at STP produced from the decomposition of 152 g CaCO3 by the reaction CaCO3(s) → CaO(s) + CO2(g) 12. A sample of methane gas having a volume of 2.80 L at 25ºC and 1.65 atm was mixed with a sample of oxygen gas having a volume of 35.0 L at 31ºC and 1.25 atm. The mixture was then ignited to form carbon dioxide and water. Calculate the volume of CO2 formed at a pressure of 2.50 atm and a temperature of 125ºC.