Question 1

This equation is used to calculate the properties of a gas under nonideal conditions.

Accepted Answer

A)  Charles's law 
B)  Avogadro's law 
C)  Boyle's law 
D)  van der Waals equation 
E)  Dalton's law 
A)  Charles's law 
B)  Avogadro's law 
C)  Boyle's law 
D)  van der Waals equation 
E)  Dalton's law

Question 2

What is the temperature of SO2 gas if the average speed (actually the root mean square speed) of the molecules is 750 m s-1?

Accepted Answer

A)  1.92 K 
B)  1.44 × 103 K 
C)  1.92 × 103 K 
D)  1.44 × 106 K 
A)  1.92 K 
B)  1.44 × 103 K 
C)  1.92 × 103 K 
D)  1.44 × 106 K

Question 3

How many molecules of N2 are in a 400.0 mL container at 1.0399 bar and 135 °C?

Accepted Answer

A)  7.01 × 1021 molecules 
B)  7.38 × 1021 molecules 
C)  2.12 × 1022 molecules 
D)  2.23 × 1022 molecules 
A)  7.01 × 1021 molecules 
B)  7.38 × 1021 molecules 
C)  2.12 × 1022 molecules 
D)  2.23 × 1022 molecules

Question 4

What is the lowest layer of the atmosphere?

Accepted Answer

A)  stratosphere 
B)  mesosphere 
C)  nanosphere 
D)  troposphere 
E)  thermosphere 
A)  stratosphere 
B)  mesosphere 
C)  nanosphere 
D)  troposphere 
E)  thermosphere

Question 5

How many moles of molecular oxygen are required to produce a pressure of 0.413 bar in a 650 mL container with a temperature of 245 K?

Accepted Answer

A)  0.0132 mol 
B)  0.199 mol 
C)  0.00872 mol 
D)  0.00971 mol 
E)  0.0245 mol 
A)  0.0132 mol 
B)  0.199 mol 
C)  0.00872 mol 
D)  0.00971 mol 
E)  0.0245 mol

Question 6

Which of the following will cause the volume of an ideal gas to triple in value?

Accepted Answer

A)  raising the temperature from 25 °C to 75 °C at constant pressure 
B)  lowering the absolute temperature by a factor of 3 at constant pressure 
C)  raising the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
D)  lowering the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
E)  lowering the pressure by a factor of 3 while the temperature stays constant 
A)  raising the temperature from 25 °C to 75 °C at constant pressure 
B)  lowering the absolute temperature by a factor of 3 at constant pressure 
C)  raising the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
D)  lowering the absolute temperature by a factor of 3 while increasing the pressure by a factor of 3 
E)  lowering the pressure by a factor of 3 while the temperature stays constant

Question 7

The volume of 350. mL of gas at 25 °C is decreased to 135 mL at constant pressure. What is the final temperature of the gas?

Accepted Answer

A)  -158 °C 
B)  9.6 °C 
C)  65 °C 
D)  500 °C 
A)  -158 °C 
B)  9.6 °C 
C)  65 °C 
D)  500 °C

Question 8

When 14.0 g of zinc metal reacts with excess HCl, how many litres of H2 gas are produced at STP?

Accepted Answer

A)  0.208 L 
B)  0.416 L 
C)  4.86 L 
D)  9.60 L 
A)  0.208 L 
B)  0.416 L 
C)  4.86 L 
D)  9.60 L

Question 9

Match the following.
-Charles'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 10

How many litres of oxygen are needed to exactly react with 19.8 g of methane at STP? 
CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

Accepted Answer

A)  13.9 L 
B)  27.8 L 
C)  56.0 L 
D)  60.5 L 
A)  13.9 L 
B)  27.8 L 
C)  56.0 L 
D)  60.5 L

Question 11

Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 bar.

Accepted Answer

A)  63.1 K 
B)  5.25 K 
C)  337 K 
D)  28.0 K 
A)  63.1 K 
B)  5.25 K 
C)  337 K 
D)  28.0 K

Question 12

Convert 4744.1 mmHg to bar.

Accepted Answer

A)  7.549 bar 
B)  5.2423 bar 
C)  5.278 bar 
D)  6.817 bar 
E)  6.325 bar 
A)  7.549 bar 
B)  5.2423 bar 
C)  5.278 bar 
D)  6.817 bar 
E)  6.325 bar

Question 13

Which of the following statements is FALSE?

Accepted Answer

A)  Real gases do not fit the assumptions of kinetic molecular theory. 
B)  The assumptions of kinetic molecular theory break down at high pressures. 
C)  The assumptions of kinetic molecular theory break down at high temperatures. 
D)  The assumptions of kinetic molecular theory break down at low temperatures. 
E)  The van der Waals equation predicts gas properties under nonideal conditions. 
A)  Real gases do not fit the assumptions of kinetic molecular theory. 
B)  The assumptions of kinetic molecular theory break down at high pressures. 
C)  The assumptions of kinetic molecular theory break down at high temperatures. 
D)  The assumptions of kinetic molecular theory break down at low temperatures. 
E)  The van der Waals equation predicts gas properties under nonideal conditions.

Question 14

Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)?

Accepted Answer

A)  15 g F2 
B)  15 g Ne 
C)  15 g Kr 
D)  15 g CO2 
E)  All of these samples will have the same pressure. 
A)  15 g F2 
B)  15 g Ne 
C)  15 g Kr 
D)  15 g CO2 
E)  All of these samples will have the same pressure.

Question 15

Explain what the term "mean free path" describes. How does it change with decreasing pressure?

Accepted Answer

Mean free path describes the distance th

Question 16

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains   flask B contains O3, and flask C contains F2. Which flask contains the largest number of molecules?

Accepted Answer

A)  flask A 
B)  flask B 
C)  flask C 
D)  All contain the same number of molecules. 
A)  flask A 
B)  flask B 
C)  flask C 
D)  All contain the same number of molecules.

Question 17

Match the following.
-manometer

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 18

The volume of a gas is proportional to number of moles of a gas. What is this known as?

Accepted Answer

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

Question 19

What is the temperature if krypton has a root mean square velocity of 348 m   ?

Accepted Answer

A)  800°C 
B)  791°C 
C)  134°C 
D)  604°C 
E)  596°C 
A)  800°C 
B)  791°C 
C)  134°C 
D)  604°C 
E)  596°C

Question 20

Which of the following samples will have the greatest volume at STP?

Accepted Answer

A)  22 g CO 
B)  22 g He 
C)  22 g O2 
D)  22 g Cl2 
E)  All of these samples would have the same volume at STP. 
A)  22 g CO 
B)  22 g He 
C)  22 g O2 
D)  22 g Cl2 
E)  All of these samples would have the same volume at STP.

Exam 5: Gases

This equation is used to calculate the properties of a gas under nonideal conditions.

What is the temperature of SO2 gas if the average speed (actually the root mean square speed) of the molecules is 750 m s-1?

How many molecules of N2 are in a 400.0 mL container at 1.0399 bar and 135 °C?

What is the lowest layer of the atmosphere?

How many moles of molecular oxygen are required to produce a pressure of 0.413 bar in a 650 mL container with a temperature of 245 K?

Which of the following will cause the volume of an ideal gas to triple in value?

The volume of 350. mL of gas at 25 °C is decreased to 135 mL at constant pressure. What is the final temperature of the gas?

When 14.0 g of zinc metal reacts with excess HCl, how many litres of H2 gas are produced at STP?

Match the following. -Charles's law

How many litres of oxygen are needed to exactly react with 19.8 g of methane at STP? CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)

Calculate the temperature, in K, of 2.20 moles of gas occupying 3.50 L at 3.30 bar.

Convert 4744.1 mmHg to bar.

Which of the following statements is FALSE?

Which of the following samples will have the lowest pressure if they are all at the same temperature and in identical containers (same volume)?

Explain what the term "mean free path" describes. How does it change with decreasing pressure?

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains flask B contains O3, and flask C contains F2. Which flask contains the largest number of molecules?

Match the following. -manometer

The volume of a gas is proportional to number of moles of a gas. What is this known as?

What is the temperature if krypton has a root mean square velocity of 348 m ?

Which of the following samples will have the greatest volume at STP?

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

What is the temperature of SO₂ gas if the average speed (actually the root mean square speed) of the molecules is 750 m s^-1?

How many molecules of N₂ are in a 400.0 mL container at 1.0399 bar and 135 °C?

When 14.0 g of zinc metal reacts with excess HCl, how many litres of H₂ gas are produced at STP?

How many litres of oxygen are needed to exactly react with 19.8 g of methane at STP? CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l)

Three identical flasks contain three different gases at standard temperature and pressure. Flask A contains flask B contains O₃, and flask C contains F₂. Which flask contains the largest number of molecules?