1. Which of the following images most accurately reflects the distribution of gas molecules in a chamber?
2. How does the downward motion of the piston in the figure below affect the pressure of the gas in the cylinder?
3. Convert a barometric reading of 30.02 in height of Hg into atm. (2.54 cm = 1 in; 10 mm = 1 cm; 760 mm Hg = 1 atm)
4. Consider the figure below. The two containers are filled with CO2 gas under the same Temperature and volume. Assume each molecule is represented by the dots. Which container will exert more Pressure under?
5. Consider the vessel below containing two gas molecules: A = light dots and B = dark dots. Which gas molecule will exert a greater partial pressure?
6. Consider the figure above containing A and B gas molecules. Calculate the mole fraction of A and the mole fraction of B.
7. Which of the following gas molecules will have a faster rate of effusion?
a. Helium gas (He)
b. CO2 gas
c. O2 gas
d. Methane (CH4) gas
e. All have the same rate
8. In which container is the gas Pressure, the least (smallest)?
9. In which container is the gas Pressure the greatest?
10. Consider the figure below where the gas flask on the left is immersed in an ice bath while the gas flask on the right is immersed in a boiling water bath. Which flask would the stopper more likely to pop out ? Why ?
11. What is STP (Standard Temperature and Pressure)?
12. Consider the reaction: 2CO(g) + O2(g) ? 2CO2(g). If one volume of CO was used in this combustion reaction, how much volume of the CO2 will be produced?
13. How much volume is contained in 1.0 mole of Ar at STP?
14. How many moles of air must there be in a racing bike tire with a volume of 2.36 L if it has an internal pressure of 6.8 atm at 17.0°C ?