Question 1

Which of the following equations shows an incorrect relationship between pressures given in terms of different units?

Accepted Answer

A)  152 mmHg = 2.03 × 104 Pa 
B)  1.20 atm = 122 kPa 
C)  1.00 atm = 760 torr 
D)  1.0 torr = 2.00 mmHg 
E)  0.760 atm = 578 mmHg 
A)  152 mmHg = 2.03 × 104 Pa 
B)  1.20 atm = 122 kPa 
C)  1.00 atm = 760 torr 
D)  1.0 torr = 2.00 mmHg 
E)  0.760 atm = 578 mmHg

Question 2

The pressure exerted by a column of liquid is equal to the product of the height of the column times the gravitational constant times the density of the liquid, P = ghd. How high a column of water (d = 1.0 g/mL) would be supported by a pressure that supports a 713 mm column of mercury (d = 13.6 g/mL)?

Accepted Answer

A)  1.2 × 104 mm 
B)  9.7 × 103 mm 
C)  14 mm 
D)  713 mm 
E)  52 mm 
A)  1.2 × 104 mm 
B)  9.7 × 103 mm 
C)  14 mm 
D)  713 mm 
E)  52 mm

Question 3

Two deviations of real gases from ideal gases which are treated in the van der Waals equation are finite molecular volume and non- zero molecular attractions.

Accepted Answer

A) True 
 B)False

Question 4

Sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas:
 
A sample of NaH weighing g will produce 982 mL of gas at 28.0 °C and 765 torr, when the hydrogen is collected over water. The vapor pressure of water at this temperature is 28 torr.

Accepted Answer

A)  925 
B)  0.0388 
C)  0.960 
D)  2.93 
E)  0.925 
A)  925 
B)  0.0388 
C)  0.960 
D)  2.93 
E)  0.925

Question 5

When gases are treated as real, via use of the van der Waals equation, the actual volume occupied by gas molecules the pressure exerted and the attractive forces between gas molecules
The pressure exerted, as compared to an ideal gas.

Accepted Answer

A)  increases, decreases 
B)  increases, increases 
C)  does not affect, increases 
D)  does not affect, decreases 
E)  decreases, increases 
A)  increases, decreases 
B)  increases, increases 
C)  does not affect, increases 
D)  does not affect, decreases 
E)  decreases, increases

Question 6

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 °C is atm. (a = 6.49 L2- atm/mol2, b = 0.0562 L/mol)

Accepted Answer

A)  0.676 
B)  1.50 
C)  1.48 
D)  0.993 
E)  1.91 
A)  0.676 
B)  1.50 
C)  1.48 
D)  0.993 
E)  1.91

Question 7

A 0.325 L flask filled with gas at 0.914 atm and 19 °C contains mol of gas.

Accepted Answer

A)  1.48 × 10- 2 
B)  12.4 
C)  80.7 
D)  1.24 × 10- 2 
E)  9.42 
A)  1.48 × 10- 2 
B)  12.4 
C)  80.7 
D)  1.24 × 10- 2 
E)  9.42

Question 8

The density of krypton gas at 1.21 atm and 50.0 °C is g/L.

Accepted Answer

A)  0.295 
B)  7.65 
C)  0.0456 
D)  3.82 
E)  0.262 
A)  0.295 
B)  7.65 
C)  0.0456 
D)  3.82 
E)  0.262

Question 9

A real gas will behave most like an ideal gas under conditions of .

Accepted Answer

A)  low temperature and low pressure 
B)  high temperature and high pressure 
C)  high temperature and low pressure 
D)  STP 
E)  low temperature and high pressure 
A)  low temperature and low pressure 
B)  high temperature and high pressure 
C)  high temperature and low pressure 
D)  STP 
E)  low temperature and high pressure

Question 10

CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was atm.

Accepted Answer

A)  4.02 
B)  10.3 
C)  1.60 
D)  0.292 
E)  6.31 
A)  4.02 
B)  10.3 
C)  1.60 
D)  0.292 
E)  6.31

Question 11

The pressure exerted by a column of liquid is equal to the product of the height of the column times the gravitational constant times the density of the liquid, P = ghd. How high a column of methanol (d = 0.79 g/mL) would be supported by a pressure that supports a 713 mm column of mercury (d = 13.6 g/mL)?

Accepted Answer

A)  1.2 × 104 mm 
B)  9.7 × 103 mm 
C)  17 mm 
D)  713 mm 
E)  41 mm 
A)  1.2 × 104 mm 
B)  9.7 × 103 mm 
C)  17 mm 
D)  713 mm 
E)  41 mm

Question 12

A sample of gas (1.9 mol) is in a flask at 21 °C and 697 mmHg. The flask is opened and more gas is added to the flask. The new pressure is 795 mmHg and the temperature is now 26 °C. There are now _ _ mol of gas in the flask.

Accepted Answer

A)  2.9 
B)  0.28 
C)  2.1 
D)  1.6 
E)  3.5 
A)  2.9 
B)  0.28 
C)  2.1 
D)  1.6 
E)  3.5

Question 13

How much faster does 235UF6 effuse than 238UF6?

Accepted Answer

A)  1.006 times as fast 
B)  1.004 times as fast 
C)  1.013 times as fast 
D)  1.009 times as fast 
E)  1.018 times as fast 
A)  1.006 times as fast 
B)  1.004 times as fast 
C)  1.013 times as fast 
D)  1.009 times as fast 
E)  1.018 times as fast

Question 14

If one was told that their blood pressure was 130/80, their systolic pressure was .

Accepted Answer

A)  130 mmHg 
B)  80 Pa 
C)  80 mmHg 
D)  130 Pa 
E)  80 psi 
A)  130 mmHg 
B)  80 Pa 
C)  80 mmHg 
D)  130 Pa 
E)  80 psi

Question 15

Which one of the following is a valid statement of Avogadro's law?

Accepted Answer

A)  PV = constant 
B)    constant 
C)  V = constant × n 
D)    constant 
E)  V = constant × P 
A)  PV = constant 
B)    constant 
C)  V = constant × n 
D)    constant 
E)  V = constant × P

Question 16

A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was atm.

Accepted Answer

A)  1.00 
B)  16.0 
C)  2.00 
D)  8.00 
E)  4.00 
A)  1.00 
B)  16.0 
C)  2.00 
D)  8.00 
E)  4.00

Question 17

A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [ P2 ] is .
P1

Accepted Answer

A)  1.50 
B)  1.13 
C)  0.882 
D)  0.667 
E)  1.00 
A)  1.50 
B)  1.13 
C)  0.882 
D)  0.667 
E)  1.00

Question 18

A sample of H2 gas (2.0 L) at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is atm. Assume the initial pressure in the flask was 0.00 atm.

Accepted Answer

A)  24 
B)  0.56 
C)  1.6 
D)  1.0 
E)  2.8 
A)  24 
B)  0.56 
C)  1.6 
D)  1.0 
E)  2.8

Question 19

The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is _ L.

Accepted Answer

A)  4.38 
B)  2.19 
C)  3.41 
D)  13.6 
E)  6.82 
A)  4.38 
B)  2.19 
C)  3.41 
D)  13.6 
E)  6.82

Question 20

The density of N2O at 1.53 atm and 45.2 °C is g/L.

Accepted Answer

A)  9.99 
B)  0.388 
C)  1.76 
D)  18.2 
E)  2.58 
A)  9.99 
B)  0.388 
C)  1.76 
D)  18.2 
E)  2.58

Exam 10: Gases

Which of the following equations shows an incorrect relationship between pressures given in terms of different units?

Two deviations of real gases from ideal gases which are treated in the van der Waals equation are finite molecular volume and non- zero molecular attractions.

Sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas: A sample of NaH weighing g will produce 982 mL of gas at 28.0 °C and 765 torr, when the hydrogen is collected over water. The vapor pressure of water at this temperature is 28 torr.

When gases are treated as real, via use of the van der Waals equation, the actual volume occupied by gas molecules the pressure exerted and the attractive forces between gas molecules The pressure exerted, as compared to an ideal gas.

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 °C is atm. (a = 6.49 L2- atm/mol2, b = 0.0562 L/mol)

A 0.325 L flask filled with gas at 0.914 atm and 19 °C contains mol of gas.

The density of krypton gas at 1.21 atm and 50.0 °C is g/L.

A real gas will behave most like an ideal gas under conditions of .

CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was atm.

A sample of gas (1.9 mol) is in a flask at 21 °C and 697 mmHg. The flask is opened and more gas is added to the flask. The new pressure is 795 mmHg and the temperature is now 26 °C. There are now _ _ mol of gas in the flask.

How much faster does 235UF6 effuse than 238UF6?

If one was told that their blood pressure was 130/80, their systolic pressure was .

Which one of the following is a valid statement of Avogadro's law?

A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was atm.

A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [ P2 ] is . P1

A sample of H2 gas (2.0 L) at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is atm. Assume the initial pressure in the flask was 0.00 atm.

The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is _ L.

The density of N2O at 1.53 atm and 45.2 °C is g/L.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Chemistry of Coordination Compounds

The Chemistry of Life: Organic and Biological Chemistry

Filters

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 °C is atm. (a = 6.49 L²- atm/mol², b = 0.0562 L/mol)

CO (5.00 g) and CO₂(5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was atm.

How much faster does ²³⁵UF₆effuse than ²³⁸UF₆?

A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [ ^P²] is . P₁

A sample of H₂gas (2.0 L) at 3.5 atm was combined with 1.5 L of N₂gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is atm. Assume the initial pressure in the flask was 0.00 atm.

The density of N₂O at 1.53 atm and 45.2 °C is g/L.