General Chemistry I (Casanova)
Assignment 4: Chapter 9
Name: _____________________________________________
1. Define the following terms: a) Pressure – b) Barometer – c) Manometer – d) Ideal Gas – e) Standard Temperature and Pressure (STP) – f) Molar volume – g) Partial pressure – h) Effusion - i) Diffusion - M/W or T/R ? Setup of each problem must be shown when performing ANY CALCULATION from this point on. Attention
should be given to significant figures. 2. Compare and contrast the three (3) states of matter with respect to the following conditions: Condition
Volume as pressure
changes
Volume as temperature
changes Solids Liquids 3. Briefly explain each of the postulates proposed by the Kinetic Molecular Theory (KMT)
Postulate 1 – Particle volume Postulate 2 – Particle motion Postulate 3 – Particle collisions 4. For Boyle’s Law:
a) State the law in words as well as mathematically b) What variables are held constant while observing the law? Gases c) A mass of oxygen occupies 5.00 L under 740 torr pressure. What is the volume of the same mass of gas
when the pressure is changed to 760 torr pressure at constant temperature? 5. For Charles’ Law:
a) State the law in words as well as mathematically b) What variables are held constant while observing the law? c) A mass of neon occupies 200 cm3 at 100oC. Find its volume at 0oC under constant pressure. 6. For the Ideal Gas Law:
a) State the law in words as well as mathematically b) State the value of the universal gas constant (R). Be sure to include all units. c) State mathematically the modified version of the ideal gas equation used to determine the molar mass of a
gaseous substance. d) State mathematically the modified version of the ideal gas equation used to determine the density in g/L for
a gaseous substance. e) Determine the volume occupied by 4.0 g of oxygen gas (O2) at S.T.P.. f) Determine the pressure of a 0.125 mole gas sample contained in a 5.00 ml container at a temperature of
350. oC g) Determine the approximate molar mass of a gas if 560 cm3 weighs 1.55g at S.T.P. h) Compute the approximate density of methane gas, CH4, at 20.0oC and 5.00 atm. 7. For the Combined Gas Law:
a) State the law mathematically b) One liter of gas, originally at 1.00 atm and -20.0oC, was warmed to 40.0oC. How many atmospheres
pressure must it then be subjected to in order to reduce its volume to 0.500 L? c) A container holds 6.00 g of CO2 at 150oC and 100 KPa pressure. How many grams of CO2 will it hold at 30oC
and the same pressure? 8. Given the following diagrams determine the pressure of the gas samples contained in each open-tube
manometer. Note that the atmospheric pressure is 760 Torr. Δh =
25.0
mm Hg
GAS SAMPLE A a) Gas sample A b) Gas sample B GAS SAMPLE B Δh = 50.0
mm Hg 9. Given the following diagram determine the pressure of the dry gaseous product (H2) as well as its mass
produced in the reaction:
Mg(s) + 2 HCl(aq) H2(g) + MgCl2(aq) VH 2 350 ml
Atmospheric pressure = 750 torr
HCl(aq)
Water level inside and outside of
the tube are the same. TH 2O 15.0o C
Mg
H2(g) 10. The gas from a certain volcano had the following composition in mole percent (i.e. mole fraction x 100):
65.0% CO2, 25.0% H2, 5.4% HCl, 2.8% HF, 1.7% SO2, and 0.1% H2S. What would be the partial pressure of
each of these gases if the total pressure of volcanic gas were 760 mmHg? 11. If a sample of N2 gas (2.0 mmol) effused through a pinhole in 5.5 s, how many seconds will it take the
same amount of CH4 gas to effuse under the same conditions? 12. A sample of He gas (2.0 mmol) effused through a pinhole in 53 s. If the same amount of an unknown gas,
under the same conditions, effused through a pinhole in 248 s determine the molecular mass of the unknown
gas. 13. How many mL of HCl(g) form at STP when 0.117 kg of sodium chloride reacts with excess sulfuric acid?
H2SO4(l) + 2 NaCl(s) Na2SO4(aq) + 2 HCl(g) 14. Pyruvic acid, HC3H3O3, is involved in cell metabolism. It can be assayed for (i.e. the amount of it
determined) by using a yeast enzyme. The enzyme makes the following reaction go to completion: HC3H3O3(aq) C2H4O(aq) + CO2(g)
If a sample containing pyruvic acid gives 21.2 ml of carbon dioxide gas at 349 mmHg and 30.0oC, how many
grams of pyruvic acid are there in the sample?

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