Download GAS PRACTICE A sample of an ideal gas is cooled from 50.0 °C to

GAS PRACTICE
1. A sample of an ideal gas is cooled from 50.0 °C to 25.0 °C in a sealed container of constant volume. Which of
the following values for the gas will decrease?
I. The average molecular mass of the gas
II. The average distance between the molecules
III. The average speed of the molecules
(A) I only
(B) II only
(C) III only
(D) I and III
(E) II and III
2. A sample of 0.010 moles of oxygen gas is confined at 127 °C and 0.80 atmospheres. What would be the pressure
of this sample at 27 °C and the same volume?
(A) 0.10 atm
(B) 0.20 atm
(C) 0.60 atm
(D) 0.80 atm
(E) 1.1 atm
3. Given the following reaction: 2 K + 2 H2O  2 K+ + 2 OH− + H2
When 0.400 moles of potassium reacts with excess water at standard temperature and pressure as shown in
the equation above, the volume of hydrogen gas produced is…
(A) 1.12 liters (B) 2.24 liters (C) 3.36 liters (D) 4.48 liters (E) 6.72 liters
4. A rigid metal tank contains oxygen gas. Which of the following applies to the gas in the tank when additional
oxygen is added at constant temperature?
(A) The volume of the gas increase.
(B) The pressure of the gas decreases.
(C) The average speed of the gas molecules remains the same.
(D) The total number of gas molecules remains the same.
(E) The average distance between the gas molecules increases.
5. NH4NO3(s)  N2O(g) + 2 H2O(g)
(Container Volume = 1.0 L)
A 0.03 mol sample of NH4NO3(s) decomposes completely according to the balanced equation above. The total
pressure in the flask measured at 400 K is closest to which of the following?
(A) 3 atm
(B) 1 atm
(C) 0.5 atm
(D) 0.1 atm
(E) 0.03 atm
6. When a sample of oxygen gas in a closed container of constant volume is heated until its absolute temperature
is doubled, which of the following is also doubled?
(A) The density of the gas
(B) The pressure of the gas
(C) The average velocity of the gas molecules
(D) The number of molecules per cm3
(E) The potential energy of the molecules
7. A compound is heated to produce a gas whose molecular weight is to be determined. The gas is collected by
displacing water in a water-filled flask inverted in a trough of water. Which of the following is necessary to
calculate the molecular weight of the gas, but does NOT need to be measured during the experiment?
(A) Mass of the compound used in the experiment
(D) Temperature of the water in the trough
(B) Vapor pressure of the water
(E) Barometric pressure
(C) Volume of water displaced from the flask
8. A sample of 3.0 grams of an ideal gas at 121°C and 1.0 atmospheres pressure has a volume of 1.5 Liters. Which
of the following expressions is correct for the molar mass of the gas?
(A) [(0.082)(394)] / [(3.0)(1.0)(1.5)]
(D) [(3.0)(0.082)(394)] / [(1.0)(1.5)]
(B) [(l.0)(l.5)] / [(3.0)(0.082)(394)]
(E) [(3.0)(0.082)(1.5)] / (1.0)(394)]
(C) [(0.082)(1.0)(1.5)] / [(3.0)(394)]
9. The density of an unknown gas is 4.20 grams per liter at 3.00 atmospheres pressure and 127 °C. What is the
molecular weight of this gas? (R = 0.0821 L-atm / mole-K)
(A) 14.6
(B) 46.0
(C) 88.0
(D) 94.1
(E) 138
10. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container. If the temperature
of the system remains constant, which of the following statements about the partial pressure of gas X is
correct?
(A) It is equal to 1/3 the total pressure
(B) It depends on the intermolecular forces of attraction between molecules of X, Y, and Z.
(C) It depends on the relative molecular masses of X, Y, and Z.
(D) It depends on the average distance traveled between molecular collisions.
(E) It can be calculated with knowledge only of the volume of the container.
11. A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.50 mole of helium exerts a
total pressure of 0.90 atmospheres. What is the partial pressure of the nitrogen?
(A) 0.13 atm (B) 0.27 atm (C) 0.63 atm (D) 0.90 atm (E) 6.3 atm
12. Hydrogen gas is collected over water at 24 °C. The total pressure of the sample is 755 millimeters of mercury.
At 24 °C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen
gas?
(A) 22 mm Hg
(B) 733 mm Hg
(C) 755 mm Hg
(D) 760 mm Hg
(E) 777 mm Hg
13. Two flexible containers for gases are at the same temperature and pressure. One holds 0.50 grams of hydrogen
and the other holds 8.0 grams of oxygen. Which of the following statements regarding these gas samples is
FALSE?
(A) The volume of the hydrogen container is the same as the volume of the oxygen container.
(B) The number of molecules in the hydrogen container is the same as the number of molecules in the oxygen
container.
(C) The density of the hydrogen sample is less than that of the oxygen sample.
(D) The average kinetic energy of the hydrogen molecules is the same as the average kinetic energy of the oxygen
molecules.
(E) The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules.
14. At 25 °C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 moles per minute. Under the same
conditions, which of the following gases effuses at approximately one-half that rate?
(A) O2 (molar mass 32 grams)
(B) He (molar mass 4.0 grams)
(C) CO2 (molar mass 44 grams)
(D) Cl2 (molar mass 71 grams)
(E) CH4 (molar mass 16 grams)
15. Equal numbers of moles of He(g), Ar(g), and Ne(g) are placed in a glass vessel at room temperature. If the vessel
has a pinhole-sized leak, which of the following will be true regarding the relative values of the partial
pressures of the gases remaining in the vessel after some of the gas mixture has effused?
(A) PHe < PNe < PAr
(B) PHe < PAr < PNe
(C) PNe < PAr < PHe
(D) PAr < PHe < PNe
(E) PHe = PAr = PNe
Questions 16 - 18 refer to the following gases at 0°C and 1 atm:
(A) Ne
(B) Xe
(C) O2
(D) CO
(E) NO
16. Has an average atomic or molecular speed closest to that of N 2 molecules at 0°C and 1 atm.
17. Has the greatest density.
18. Has the greatest rate of effusion through a pinhole.
19. When the actual gas volume is greater than the volume predicted by the ideal gas law, the explanation lies in
the fact that the ideal gas law does NOT include a factor for molecular…
(A) volume
(B) mass
(C) velocity
(D) attractions
(E) shape
20. Which of the following gases deviates most from ideal behavior?
A) SO2
B) Ne
C) CH4
D) N2
E) H2
21. A student collected a sample of hydrogen gas by the displacement of water as shown by the diagram above.
The relevant data are given below:
Volume of sample = 90.0 mL
Temperature = 25°C
Atmospheric Pressure = 745 mmHg
Equilibrium Vapor Pressure of water at 25°C = 23.8 mmHg
(a) Calculate the number of moles of hydrogen gas collected.
(b) Calculate the ratio of the average speed of the hydrogen molecules to the average speed of the water vapor
molecules in the sample.
(c) Which of the two gases, H2 or H2O, deviates more from ideal behavior? Explain your answer.
22. Answer the following questions about carbon monoxide, CO(g), and carbon dioxide, CO 2(g). Assume that both
gases exhibit ideal behavior.
(a) Draw the complete Lewis structure (electron-dot diagram) for the CO molecule and for the CO2 molecule.
(b) Identify the shape of the CO2 molecule.
(c) A 1.0 mole sample of CO(g) is heated at constant pressure. On the graph
sketch the expected plot of volume versus temperature as the gas is heated.
(e) Samples of CO(g) and C02(g) are placed in 1 L containers at the conditions indicated in the diagram below.
(i) Indicate whether the average kinetic energy of the C0 2(g) molecules is greater than, equal to, or less than the
average kinetic energy of the CO(g) molecules. Justify your answer.
(ii) Indicate whether the root-mean-square speed of the CO2(g) molecules is greater than, equal to, or less than the
root-mean-square speed of the CO(g) molecules. Justify your answer.
(iii) Indicate whether the number of CO2(g) molecules is greater than, equal to, or less than the number of CO(g)
molecules. Justify your answer.
IMF PRACTICE
1. Which of the following actions would be likely to change the boiling point of a sample of a pure liquid in
an open container?
I. Placing it in a smaller container
II. Increasing the number of moles of the liquid in the container
III. Moving the container and liquid to a higher altitude
(A) I only
(B) II only
(C) III only
(D) II and III only
(E) I, II, and III
Questions 2-5 refer to the following descriptions of bonding in different types of solids.
(A) Lattice of positive and negative ions held together by electrostatic forces
(B) Closely packed lattice with delocalized electrons throughout
(C) Strong single covalent bonds with weak intermolecular forces
(D) Strong multiple covalent bonds (including bonds.) with weak intermolecular forces
(E) Macromolecules held together with strong polar bonds
2. Cesium chloride, CsCl (s)
3. Gold, Au(s)
4. Carbon dioxide, CO2(s)
5. Methane, CH4(s)
Questions 6-7 relate to the graph shown on the right. The graph shows the temperature of a pure substance as it
is heated at a constant rate in an open vessel at 1.0 atm pressure. The substance changes from the solid to the
liquid to the gas phase.
6. The substance is at its normal freezing point at time…
15. (A) t1 (B) t2 (C) t3
(D) t4
(E) t5
7. Which of the following best describes what happens to the
substance between t4 and t5?
(A) The molecules are leaving the liquid phase.
(B) The solid and liquid phases coexist in the equilibrium.
(C) The vapor pressure of the substance is decreasing.
(D) The average intermolecular distance is decreasing.
(E) The temperature of the substance is increasing.
8. The best explanation for the fact that diamond is extremely hard is that diamond crystals…
(A) are made up of atoms that are intrinsically hard because of their electronic structures
(B) consist of positive and negative ions that are strongly attracted to each other
(C) are giant molecules in which each atom forms strong covalent bonds with all of its neighboring atoms
(D) are formed under extreme conditions of temperature and pressure
(E) contain orbitals or bands of delocalized electrons that belong not to single atoms but to each crystal as a
whole
9. Sodium chloride is LEAST soluble in which of the following liquids?
(A) H2O (B) CCl4 (C) HF (D) CH3OH (E) CH3COOH
10. Which of the following describes the changes in forces of attraction that occur as H2O changes phase from a
liquid to a vapor?
(A) H-O bonds break as H-H and O-O bonds form.
(B) Hydrogen bonds between H2O molecules are broken.
(C) Covalent bonds between H2O molecules are broken.
(D) Ionic bonds between H+ ions and OH− ions are broken.
(E) Covalent bonds between H+ ions and H2O molecules become more effective.
11. Of the following pure substances, which has the highest melting point?
(A) S8 (B) I2 (C) SiO2 (D) SO2 (E) C6H6
12. Which of the following statements is false?
a. Condensed states have much higher densities than gases.
b. Molecules are very far apart in gases and closer together in liquids and solids.
c. Gases completely fill any container they occupy and are easily compressed.
d. Vapor refers to a gas formed by evaporation of a liquid or sublimation of a solid.
e. Solid water (ice), unlike most substances, is denser than its liquid form (water).
13. Ten (10.0) moles of a gas are contained in a 10.0 L container at 273 K. Calculate the pressure of the gas.
a. 2.24 atm
b. 4.48 atm
c. 11.2 atm
d. 15.7 atm
e. 22.4 atm
14. A mixture of gas consists of 5.0 g CH4, 5.0 g C2H2, and 5.0 g C2H4. What are the mole fractions of each?
XCH4 XC2H2 XC2H4
a. 0.321 0.192 0.177
b. 0.333 0.333 0.333
c. 0.217 0.375 0.408
d. 0.567 0.137 0.326
e. 0.457 0.281 0.262
15. A 5.00 L container contains CH4, H2, and Xe at 35 C with a total pressure of 1.81 atm. If there are equal moles of
each gas, what is the partial pressure of H2?
a. 0.603 atm
b. 0.034 atm
c. 1.81 atm
d. 3.05 atm
e. 0.362 atm
16. What is the pressure exerted by a mixture of 1.0 g H2 and 5.0 g He when confined to a volume of 5.0 liters at
20. C?
a. 12.6 atm
b. 8.4 atm
c. 3.61 atm
d. 10.4 atm
e. 6.5 atm
17. Which one of the following statements is not consistent with the kinetic-molecular theory?
a. The volume occupied by the molecules (only) of a gas becomes significant only at very low pressures.
b. A given sample of a gas is mostly empty space except near the liquefaction point.
c. Except near the liquefaction point, the attractive forces between molecules of a gas are very small.
d. Collisions between the molecules of a gas are elastic.
e. The attractive forces between the molecules of a gas become significant only at very low temperatures.
18. In terms of energy and entropy, systems in nature tend to favor changes that lead to
a. higher energy and higher entropy
b. higher energy and lower entropy
c. lower energy and higher entropy
d. lower energy and lower entropy
19. The boiling points of the halogens increase in the order F2 < Cl2 < Br2 < I2 due to the resulting increasing
__________ interactions.
a. ion-dipole
b. hydrogen-bonding
c. ion-ion
d. dispersion forces
e. permanent dipole-dipole
20. Calculate the amount of heat (in joules) required to convert 92.5 g of water at 25.0 C to steam at 108.0 C.
(Sp. heat of H2O(l) = 4.18 J/g• C, Sp. heat of H2O(g) = 2.03 J/g• C, heat of vap. of H2O(l) = 2.260 kJ/g)
SOLUTION PRACTICE
1. 150 mL of a 2.5 M magnesium nitrate is mixed with 230 mL of 1.3 M sodium phosphate. How many grams of
precipitate will be formed? What is the concentration of each ion remaining in solution after the reaction?
2. When 70. milliliters of 3.0-molar Na2CO3 is added to 30. milliliters of 1.0-molar NaHCO3 the resulting
concentration of Na+ is…
(A) 2.0 M (B) 2.4 M (C) 4.0 M (D) 4.5 M (E) 7.0 M
3. A student wishes to prepare 2.00 liters of 0.100-molar KIO3 (molecular weight 214). The proper procedure is to
weigh out…
(A) 42.8 grams of KIO3 and add 2.00 kilograms of H2O
(B) 42.8 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters
(C) 21.4 grams of KIO3 and add H2O until the final homogeneous solution has a volume of 2.00 liters
(D) 42.8 grams of KIO3 and add 2.00 liters of H2O
(E) 21.4 grams fo KIO3 and add 2.00 liters of H2O
4. A 20.0-milliliter sample of 0.200-molar K2CO3 solution is added to 30.0 milliliters of 0.400-molar Ba(NO3)2
solution. Barium carbonate precipitates. The concentration of barium ion, Ba 2+, in solution after reaction is…
(A) 0.150 M
(B) 0.160 M
(C) 0.200 M
(D) 0.240 M
(E) 0.267 M
5. The weight of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution is…
(A) 3.10 grams
(B) 12.0 grams
(C) 29.4 grams
(D) 294 grams
(E) 300. Grams
6. How many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl?
(A) 3.9 mL
(B) 35 mL
(C) 260 mL
(D) 1,000 mL
(E) 3,900 mL
7. Which of the following does NOT behave as an electrolyte when it is dissolved in water?
(A) CH3OH
(B) K2CO3 (C) NH4Br
(D) HI
(E) Sodium acetate, CH3COONa
8. How many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20-molar Fe(NO3)3 to increase the
concentration of the NO3− ion to 1.0-molar? (Assume that the volume of the solution remains constant.)
(A) 0.060 mole (B) 0.12 mole (C) 0.24 mole (D) 0.30 mole (E) 0.40 mole
9. Which of the following has the lowest conductivity?
(A) 0.1 M CuSO4 (B) 0.1 M KOH
(C) 0.1 M BaCl2 (D) 0.1 M HF
(E) 0.1 M HNO3
10. A 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. What is the minimum
number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl − as AgCl(s) ?
(Assume that AgCl is insoluble.)
(A) 0.10 mol
(B) 0.20 mol
(C) 0.30 mol
(D) 0.40 mol
(E) 0.60 mol
11. A 40.0 mL sample of 0.25 M KOH is added to 60.0 mL of 0.15 M Ba(OH) 2. What is the molar concentration of
OH−(aq) in the resulting solution? (Assume that the volumes are additive.)
(A) 0.10 M
(B) 0.19 M
(C) 0.28 M
(D) 0.40 M
(E) 0.55 M
12. The volume of distilled water that should be added to 10.0 mL of 6.00 M HCl (aq) in order to prepare a 0.500 M
HCl(aq) solution is approximately…
(A) 50.0 mL
(B) 60.0 mL
(C) 100. mL
(D) 110. mL
(E) 120. mL
13. Approximately what mass of CuSO4·5H2O (250 g mol-1) is required to prepare 250 mL of 0.10 M copper (II)
sulfate solution?
(A) 4.0 g
(B) 6.2 g (C) 34 g
(D) 85 g
(E) 140 g
14. What is the mole fraction of ethanol, C2H5OH, in an aqueous solution that is 46 percent ethanol by mass? (The
molar mass of C2H5OH is 46 g; the molar mass of H2O is 18 g.)
(A) 0.25
(B) 0.46
(C) 0.54
(D) 0.67
(E) 0.75
15. At 20 °C, the vapor pressure of toluene is 22 millimeters of mercury and that of benzene is 75 millimeters of
mercury. An ideal solution, equimolar in toluene and benzene, is prepared. At 20 °C, what is the mole fraction of
benzene in the vapor in equilibrium with this solution?
(A) 0.23
(B) 0.29
(C) 0.50
(D) 0.77
(E) 0.83
16. Which of the following aqueous solutions has the highest boiling point?
(A) 0.10 M potassium sulfate, K2SO4
(B) 0.10 M hydrochloric acid, HCl
(C) 0.10 M ammonium nitrate, NH4NO3 (D) 0.10 M magnesium sulfalte, MgSO4
(E) 0.20 M sucrose, C12H22O11
17. If the temperature of an aqueous solution of NaCl is increased from 20 °C to 90 °C, which of the following
statements is true?
(A) The density of the solution remains unchanged.
(B) The molarity of the solution remains unchanged.
(C) The molality of the solution remains unchanged. (D) The mole fraction of solute decreases.
(E) The mole fraction of solute increases.
18. A solution is made by dissolving a nonvolatile solute in pure solvent. Compared to the pure solvent, the
solution…
(A) has a higher normal boiling point.
(B) has a higher vapor pressure.
(C) has the same vapor pressure.
(D) has a higher freezing point.
(E) is more nearly ideal.
19. Below are the three steps that take place during the dissolving process. Label each as endothermic or
exothermic.
(A) Separating the solute particles
(B) Separating the solvent particles
(C) Interaction of solute and solvent particles
20. Given the answer to the above, what situation would result in a net endothermic process? Net exothermic
process?
21. If 200. mL of 0.60 M MgCl2(aq) is added to 400. mL of distilled water, what is the concentration of Mg 2+(aq) in the
resulting solution? (Assume volume are additive.)
(A) 0.20 M (B) 0.30 M (C) 0.40 M (D) 0.60 M (E) 1.2 M
22. A 0.10 M aqueous solution of sodium sulfate, Na2SO4, is a better conductor of electricity than a 0.10 M
aqueous solution of sodium chloride, NaCl. Which of the following best explains this observation?
(A) Na2SO4 is more soluble in water than NaCl is.
(B) Na2SO4 has a higher molar mass than NaCl has.
(C) To prepare a given volume of 0.10 M solution, the mass of Na 2SO4 needed is more than twice the mass of NaCl
needed.
(D) More moles of ions are present in a given volume of 0.10 M Na 2SO4 than in the same volume of 0.10 M NaCl.
(E) The degree of dissociation of Na2SO4 in solution is significantly greater than that of NaCl.
23. On the basis of the solubility curves shown, the greatest percentage of which
compound can be recovered by cooling a saturated solution of that compound
from 90°C to 30°C ?
(A) NaCl
(B) KNO3
(C) K2CrO4
(D) K2SO4
(E) Ce2(SO4)3