Question 1

A sample of an ideal gas (3.00 L)in a closed container at 25.0 °C and 76.0 torr is heated to 270 °C. The pressure of the gas at this temperature is ________ torr.

Accepted Answer

A) 912 
B) 138 
C) 76.5 
D) 39.5 
E) 0.0253 
A) 912 
B) 138 
C) 76.5 
D) 39.5 
E) 0.0253

Question 2

Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → Zn SO4 (aq) + H2 (g)
In an experiment, 201 mL of wet H2 is collected over water at 27 °C and a barometric pressure of 765 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27 °C is 26.74 torr.

Accepted Answer

A) 4.38 × 106 
B) 0.519 
C) 519 
D) 394 
E) 3.94 × 105 
A) 4.38 × 106 
B) 0.519 
C) 519 
D) 394 
E) 3.94 × 105

Question 3

A 255 mL round-bottom flask is weighed and found to have a mass of 114.85 g. A few milliliters of an easily vaporized liquid are added to the flask and the flask is immersed in a boiling water bath. All of the liquid vaporizes at the boiling temperature of water, filling the flask with vapor. When all of the liquid has vaporized, the flask is removed from the bath, cooled, dried, and reweighed. The new mass of the flask and the condensed vapor is 115.23 g. Which of the following compounds could the liquid be? (Assume the ambient pressure is 1 atm.)

Accepted Answer

A) C4H10 
B) C3H7OH 
C) C2H6 
D) C2H5OH 
E) C4H9OH 
A) C4H10 
B) C3H7OH 
C) C2H6 
D) C2H5OH 
E) C4H9OH

Question 4

SO2 (5.00 g)and CO2 (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO2 in the container was ________ atm.

Accepted Answer

A) 6.78 
B) 2.76 
C) 1.60 
D) 0.192 
E) 4.02 
A) 6.78 
B) 2.76 
C) 1.60 
D) 0.192 
E) 4.02

Question 5

A sample of He gas (3.0 L)at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.

Accepted Answer

A) 2.6 
B) 9.2 
C) 1.0 
D) 3.7 
E) 24 
A) 2.6 
B) 9.2 
C) 1.0 
D) 3.7 
E) 24

Question 6

The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is ________ g/L.

Accepted Answer

A) 3.86 
B) 0.719 
C) 0.432 
D) 0.194 
E) 4.22 × 10-2 
A) 3.86 
B) 0.719 
C) 0.432 
D) 0.194 
E) 4.22 × 10-2

Question 7

The reaction of 25 mL of N2 gas with 75 mL of H2 gas to form ammonia via the equation: N2 (g) + 3H2 (g) → 2NH3 (g)
Will produce ________ mL of ammonia if pressure and temperature are kept constant.

Accepted Answer

A) 250 
B) 50 
C) 200 
D) 150 
E) 100 
A) 250 
B) 50 
C) 200 
D) 150 
E) 100

Question 8

Of the following gases, ________ will have the greatest rate of effusion at a given temperature.

Accepted Answer

A) NH3 
B) CH4 
C) Ar 
D) HBr 
E) HCl 
A) NH3 
B) CH4 
C) Ar 
D) HBr 
E) HCl

Question 9

Standard temperature and pressure (STP), in the context of gases, refers to ________.

Accepted Answer

A) 298.15 K and 1 atm 
B) 273.15 K and 1 atm 
C) 298.15 K and 1 torr 
D) 273.15 K and 1 pascal 
E) 273.15 K and 1 torr 
A) 298.15 K and 1 atm 
B) 273.15 K and 1 atm 
C) 298.15 K and 1 torr 
D) 273.15 K and 1 pascal 
E) 273.15 K and 1 torr

Question 10

The rms speed of methane molecules at 45.0 °C is ________ m/sec.

Accepted Answer

The answer of The rms speed of methane molecules at...

Question 11

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

Accepted Answer

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

Question 12

A gas vessel is attached to an open-end manometer filled with a nonvolatile liquid of density 0.993 g/mL as shown below.   The difference in heights of the liquid in the two sides of the manometer is 32.3 mm when the atmospheric pressure is 765 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is ________ atm.

Accepted Answer

A) 1.05 
B) 1.01 
C) 0.976 
D) 0.993 
E) 1.08 
A) 1.05 
B) 1.01 
C) 0.976 
D) 0.993 
E) 1.08

Question 13

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 [   ] is ________.

Accepted Answer

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

Question 14

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

Question 15

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 16

The density of chlorine gas at 1.01 atm and 54.1 °C is ________ g/L.

Accepted Answer

A) 0.0376 
B) 0.375 
C) 0.228 
D) 1.33 
E) 2.67 
A) 0.0376 
B) 0.375 
C) 0.228 
D) 1.33 
E) 2.67

Question 17

The reaction of 50 mL of N2 gas with 150 mL of H2 gas to form ammonia via the equation: N2 (g) + 3H2 (g) → 2NH3 (g)
Will produce ________ mL of ammonia if pressure and temperature are kept constant.

Accepted Answer

A) 250 
B) 50 
C) 200 
D) 150 
E) 100 
A) 250 
B) 50 
C) 200 
D) 150 
E) 100

Question 18

Given the equation:
C2H6 (g) + O2 (g)→ CO2 (g) + H2O (g) (not balanced)
Determine the number of liters of CO2 formed at STP when 270.0 grams of C2H6 is burned in excess oxygen gas.

Accepted Answer

Question 19

What is the density (in g/L)of oxygen gas at 77.0 °C and 700.0 torr?

Accepted Answer

The answer of What is the density (in g/L)of oxygen...

Question 20

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0 °C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce ________ L of CO2.

Accepted Answer

A) 1.09 × 102 
B) 2.85 × 104 
C) 1.82 × 104 
D) 8.70 × 102 
E) 1.82 × 103 
A) 1.09 × 102 
B) 2.85 × 104 
C) 1.82 × 104 
D) 8.70 × 102 
E) 1.82 × 103

A sample of an ideal gas (3.00 L)in a closed container at 25.0 °C and 76.0 torr is heated to 270 °C. The pressure of the gas at this temperature is ________ torr.

SO₂ (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO₂ in the container was ________ atm.

A sample of He gas (3.0 L)at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.

The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is ________ g/L.

The reaction of 25 mL of N₂ gas with 75 mL of H₂ gas to form ammonia via the equation: N₂ (g) + 3H₂ (g) → 2NH₃ (g) Will produce ________ mL of ammonia if pressure and temperature are kept constant.

Of the following gases, ________ will have the greatest rate of effusion at a given temperature.

Standard temperature and pressure (STP), in the context of gases, refers to ________.

The rms speed of methane molecules at 45.0 °C is ________ m/sec.

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

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 [ ] is ________.

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.

The density of chlorine gas at 1.01 atm and 54.1 °C is ________ g/L.

The reaction of 50 mL of N₂ gas with 150 mL of H₂ gas to form ammonia via the equation: N₂ (g) + 3H₂ (g) → 2NH₃ (g) Will produce ________ mL of ammonia if pressure and temperature are kept constant.

Given the equation: C₂H₆(g) + O₂ (g)→ CO₂ (g) + H₂O (g) (not balanced) Determine the number of liters of CO₂ formed at STP when 270.0 grams of C₂H₆ is burned in excess oxygen gas.

What is the density (in g/L)of oxygen gas at 77.0 °C and 700.0 torr?

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0 °C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce ________ L of CO₂.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

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Exam 10: Gases

A sample of an ideal gas (3.00 L)in a closed container at 25.0 °C and 76.0 torr is heated to 270 °C. The pressure of the gas at this temperature is ________ torr.

SO2 (5.00 g)and CO2 (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO2 in the container was ________ atm.

A sample of He gas (3.0 L)at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.

The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is ________ g/L.

The reaction of 25 mL of N2 gas with 75 mL of H2 gas to form ammonia via the equation: N2 (g) + 3H2 (g) → 2NH3 (g) Will produce ________ mL of ammonia if pressure and temperature are kept constant.

Of the following gases, ________ will have the greatest rate of effusion at a given temperature.

Standard temperature and pressure (STP), in the context of gases, refers to ________.

The rms speed of methane molecules at 45.0 °C is ________ m/sec.

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

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 [ ] is ________.

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.

The density of chlorine gas at 1.01 atm and 54.1 °C is ________ g/L.

The reaction of 50 mL of N2 gas with 150 mL of H2 gas to form ammonia via the equation: N2 (g) + 3H2 (g) → 2NH3 (g) Will produce ________ mL of ammonia if pressure and temperature are kept constant.

Given the equation: C2H6 (g) + O2 (g)→ CO2 (g) + H2O (g) (not balanced) Determine the number of liters of CO2 formed at STP when 270.0 grams of C2H6 is burned in excess oxygen gas.

What is the density (in g/L)of oxygen gas at 77.0 °C and 700.0 torr?

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0 °C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce ________ L of CO2.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

SO₂ (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO₂ in the container was ________ atm.

The reaction of 25 mL of N₂ gas with 75 mL of H₂ gas to form ammonia via the equation: N₂ (g) + 3H₂ (g) → 2NH₃ (g) Will produce ________ mL of ammonia if pressure and temperature are kept constant.

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

The reaction of 50 mL of N₂ gas with 150 mL of H₂ gas to form ammonia via the equation: N₂ (g) + 3H₂ (g) → 2NH₃ (g) Will produce ________ mL of ammonia if pressure and temperature are kept constant.

Given the equation: C₂H₆(g) + O₂ (g)→ CO₂ (g) + H₂O (g) (not balanced) Determine the number of liters of CO₂ formed at STP when 270.0 grams of C₂H₆ is burned in excess oxygen gas.

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0 °C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce ________ L of CO₂.