Chapter 13 Gas Laws Vocabulary Assignment

Chapter 13 Gas Laws Vocabulary Assignment
Boyle’s Law
Absolute zero Charles’s Law
Ideal Gas Law
Ideal Gas
Dalton’s law of partial pressure
standard atmosphere
Avogadro’s Law
Universal Gas Constant
Combined Gas Law
Partial pressure
Kinetic molecular theory
Molar volume
Standard Temperature and Pressure
Reading Questions:
1. How are the three states of matter similar and how do they differ?
2. What is meant by “the pressure of the atmosphere”? What causes this pressure?
3. Describe a simple mercury barometer. How is such a barometer used to measure the pressure
of the atmosphere?
4. Convert the following pressures into ATMOSPHERES: 105.2 kPa, 75.2 cm Hg, 752 mm Hg, 767
5. Convert the following pressures into units of mm of Hg: 0.9975 atm, 225,400 Pa, 99.7 kPa,
1.078 atm.
6. Convert the following pressures into pascals: 774 torr, 0.965 atm, 112.5 kPa, 801 mm Hg.
7. If the pressure exerted on the gas in a weather balloon decreases from 1.01 atm to 0.562 atm as
it rises, by what factor will the volume of the gas in the balloon increase as it rises?
8. What is meant by the absolute zero of temperature?
9. If 5.00L of an ideal gas is cooled from 24oC to -272oC, what will the volume of the gas become?
10. If 46.2 g of oxygen gas occupies a volume of 100.L at a particular temperature and pressure,
what volume will 5.00g of oxygen gas occupy under the same conditions?
11. Under what conditions to REAL gases behave most ideally?
12. What volume does 4.24g of nitrogen gas occupy at 58.2oC and 2.04 atm?
13. Determine the pressure in a 125-L tank containing 56.2 kg of oxygen gas at 21oC.
14. Explain why the measured properties of a mixture of gases depend only on the total number of
moles of particles, not on the identities of the individual gas particles. How is this observation
summarized as a law?
15. A tank contains a mixture of 3.0 mol N2, 2.0 mol O2, and 1.0 mol CO2 at 25oC and a total pressure
of 10.0 atm. Calculate the partial pressure (in torr) of each gas in the mixture.
16. Given the following UNBALANCED chemical equation for the combination reaction of sodium
metal and chlorine gas, what volume of chlorine gas, measured at STP, is necessary for the
complete reaction of 4.81g of sodium metal?
Na(s) + Cl2(g)