Question 1

Which of the gases in the graph below has the smallest molar mass?

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  There is not enough information to determine the answer. 
A)  A 
B)  B 
C)  C 
D)  D 
E)  There is not enough information to determine the answer.

Question 2

Which of the following gases has the highest root mean square velocity at constant temperature?

Accepted Answer

A)  NH3 
B)  CO2 
C)  NO2 
D)  F2 
E)  O3 
A)  NH3 
B)  CO2 
C)  NO2 
D)  F2 
E)  O3

Question 3

A syringe contains 589 mL of CO at 325 K and 1.2 bar. A second syringe contains 473 mL of N2 at 298 K and 2.6 bar. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at 273 K?

Accepted Answer

A)  0.59 bar 
B)  1.1 bar 
C)  1.7 bar 
D)  1.9 bar 
E)  3.8 bar 
A)  0.59 bar 
B)  1.1 bar 
C)  1.7 bar 
D)  1.9 bar 
E)  3.8 bar

Question 4

Which of the gases in the graph below has the largest molar mass?

Accepted Answer

A)  A 
B)  B 
C)  C 
D)  D 
E)  There is not enough information to determine the answer. 
A)  A 
B)  B 
C)  C 
D)  D 
E)  There is not enough information to determine the answer.

Question 5

Why does hot air rise?

Accepted Answer

As air is heated, it expands a

Question 6

Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction. The molar mass for KClO3 is 122.55 g mol-1. 2KClO3(s) → 2KCl(s) + 3O2(g)

Accepted Answer

A)  9.14 L 
B)  8.22 L 
C)  12.3 L 
D)  13.9 L 
E)  14.6 L 
A)  9.14 L 
B)  8.22 L 
C)  12.3 L 
D)  13.9 L 
E)  14.6 L

Question 7

To what volume will a sample of gas expand if it is heated from 50.0 °C and 2.33 L to 500.0 °C?

Accepted Answer

A)  5.58 L 
B)  9.74 L 
C)  10.3 L 
D)  17.9 L 
E)  4.38 L 
A)  5.58 L 
B)  9.74 L 
C)  10.3 L 
D)  17.9 L 
E)  4.38 L

Question 8

Match the following.
-Ideal gas law

Accepted Answer

A) PV = nRT 
B) V1/T1 = V2/T2 
C) V1/n1 = V2/n2 
D) PT = PA + PB + PC ... 
E) measures pressure of a gas
F)measures atmospheric pressure
G)measures blood pressure
H)P1V1 = P2V2 
A) PV = nRT 
B) V1/T1 = V2/T2 
C) V1/n1 = V2/n2 
D) PT = PA + PB + PC ... 
E) measures pressure of a gas
F)measures atmospheric pressure
G)measures blood pressure
H)P1V1 = P2V2

Question 9

Convert 717.28 mmHg to bar.

Accepted Answer

A)  1.046 bar 
B)  0.9438 bar 
C)  1.060 bar 
D)  0.9563 bar 
E)  0.8971 bar 
A)  1.046 bar 
B)  0.9438 bar 
C)  1.060 bar 
D)  0.9563 bar 
E)  0.8971 bar

Question 10

A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.43 bar. What is the identity of the halogen?

Accepted Answer

A)  Br2 
B)  F2 
C)  Cl2 
D)  I2 
E)  At2 
A)  Br2 
B)  F2 
C)  Cl2 
D)  I2 
E)  At2

Question 11

According to Avogadro's law, the volume of a gas sample ________ with an increase in the number of moles of gas in the sample. Avogadro's law assumes constant temperature and constant pressure and is independent of the identity of the gas.

Accepted Answer

A)  decreases 
B)  increases 
C)  doesn't change 
D)  increases and then decreases 
E)  decreases and then increases 
A)  decreases 
B)  increases 
C)  doesn't change 
D)  increases and then decreases 
E)  decreases and then increases

Question 12

What volume would 1.02 moles of Kr occupy at a pressure of 1.65 bar and a temperature of 281.2 K?

Accepted Answer

A)  28.7 L 
B)  14.5 L 
C)  12.7 L 
D)  6.87 L 
E)  16.9 L 
A)  28.7 L 
B)  14.5 L 
C)  12.7 L 
D)  6.87 L 
E)  16.9 L

Question 13

You have three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at -15 °C, cylinder B is at -5 °F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen?

Accepted Answer

A)  cylinder A 
B)  cylinder B 
C)  cylinder C 
D)  All cylinders contain the same mass of O2. 
A)  cylinder A 
B)  cylinder B 
C)  cylinder C 
D)  All cylinders contain the same mass of O2.

Question 14

Identify the gas particle that travels the fastest.

Accepted Answer

A)  H2 
B)  O2 
C)  Ne 
D)  N2 
E)  CO 
A)  H2 
B)  O2 
C)  Ne 
D)  N2 
E)  CO

Question 15

Match the following.
-Dalton's law

Accepted Answer

A) PV = nRT 
B) V1/T1 = V2/T2 
C) V1/n1 = V2/n2 
D) PT = PA + PB + PC ... 
E) measures pressure of a gas
F)measures atmospheric pressure
G)measures blood pressure
H)P1V1 = P2V2 
A) PV = nRT 
B) V1/T1 = V2/T2 
C) V1/n1 = V2/n2 
D) PT = PA + PB + PC ... 
E) measures pressure of a gas
F)measures atmospheric pressure
G)measures blood pressure
H)P1V1 = P2V2

Question 16

Define effusion.

Accepted Answer

Effusion is the proc

Question 17

Which one of the following gas laws explains the increase in volume of a basketball upon inflating it at constant temperature and constant pressure?

Accepted Answer

A)  Boyle's law 
B)  Avogadro's law 
C)  Charles's law 
D)  Ideal gas law 
E)  Inert gas law 
A)  Boyle's law 
B)  Avogadro's law 
C)  Charles's law 
D)  Ideal gas law 
E)  Inert gas law

Question 18

A fixed amount of gas at 25.0 °C occupies a volume of 20.0 L when the pressure is 0.8386 bar. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to   while maintaining the pressure at 0.8386 bar.

Accepted Answer

A)  14.8 L 
B)  105 L 
C)  3.82 L 
D)  22.4 L 
E)  27.1 L 
A)  14.8 L 
B)  105 L 
C)  3.82 L 
D)  22.4 L 
E)  27.1 L

Question 19

A container filled with gas is connected to an open-end manometer that is filled with mineral oil. The pressure in the gas container is 753 mmHg and atmospheric pressure is 724 mmHg. How high will the level rise in the manometer if the densities of Hg and mineral oil are 13.6 g mL-1 and 0.822 g mL-1, respectively?

Accepted Answer

A)  1.75 mm 
B)  23.8 mm 
C)  29.0 mm 
D)  480 mm 
A)  1.75 mm 
B)  23.8 mm 
C)  29.0 mm 
D)  480 mm

Question 20

If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions, what volume will 0.66 moles occupy under the same conditions?

Accepted Answer

A)  12 L 
B)  8.6 L 
C)  17 L 
D)  5.0 L 
E)  15 L 
A)  12 L 
B)  8.6 L 
C)  17 L 
D)  5.0 L 
E)  15 L

Exam 5: Gases

Which of the gases in the graph below has the smallest molar mass?

Which of the following gases has the highest root mean square velocity at constant temperature?

A syringe contains 589 mL of CO at 325 K and 1.2 bar. A second syringe contains 473 mL of N2 at 298 K and 2.6 bar. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at 273 K?

Which of the gases in the graph below has the largest molar mass?

Why does hot air rise?

Determine the volume of O2 (at STP) formed when 50.0 g of KClO3 decomposes according to the following reaction. The molar mass for KClO3 is 122.55 g mol-1. 2KClO3(s) → 2KCl(s) + 3O2(g)

To what volume will a sample of gas expand if it is heated from 50.0 °C and 2.33 L to 500.0 °C?

Match the following. -Ideal gas law

Convert 717.28 mmHg to bar.

A 0.334 g sample of an unknown halogen occupies 109 mL at 398 K and 1.43 bar. What is the identity of the halogen?

According to Avogadro's law, the volume of a gas sample ________ with an increase in the number of moles of gas in the sample. Avogadro's law assumes constant temperature and constant pressure and is independent of the identity of the gas.

What volume would 1.02 moles of Kr occupy at a pressure of 1.65 bar and a temperature of 281.2 K?

You have three cylinders containing O2 gas at the same volume and pressure. Cylinder A is at -15 °C, cylinder B is at -5 °F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen?

Identify the gas particle that travels the fastest.

Match the following. -Dalton's law

Define effusion.

Which one of the following gas laws explains the increase in volume of a basketball upon inflating it at constant temperature and constant pressure?

A fixed amount of gas at 25.0 °C occupies a volume of 20.0 L when the pressure is 0.8386 bar. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to while maintaining the pressure at 0.8386 bar.

If a sample of 0.29 moles of Ar occupies 3.8 L under certain conditions, what volume will 0.66 moles occupy under the same conditions?

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules, Compounds, and Nomenclature

Chemical Reactions and Stoichiometry

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry Ii: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

A syringe contains 589 mL of CO at 325 K and 1.2 bar. A second syringe contains 473 mL of N₂ at 298 K and 2.6 bar. What is the final pressure if the contents of these two syringes are injected into a 1.00 L container at 273 K?

Determine the volume of O₂ (at STP) formed when 50.0 g of KClO₃ decomposes according to the following reaction. The molar mass for KClO₃is 122.55 g mol^-1. 2KClO₃(s) → 2KCl(s) + 3O₂(g)

You have three cylinders containing O₂ gas at the same volume and pressure. Cylinder A is at -15 °C, cylinder B is at -5 °F, cylinder C is at 255 K. Which cylinder contains the largest mass of oxygen?