Question 1

Which one of these gases is "lighter-than-air"?

Accepted Answer

A) Cl2 
B) SO2 
C) PH3 
D) NO2 
E) Ne 
A) Cl2 
B) SO2 
C) PH3 
D) NO2 
E) Ne

Question 2

On a spring morning (20°C)you fill your tires to a pressure of 2.25 atmospheres. As you ride along, the tire heats up to 45°C from the friction on the road. What is the pressure in your tires now?

Accepted Answer

The answer of On a spring morning (20°C)you fill your...

Question 3

A sample of N2 gas occupies 2.40 L at 20°C. If the gas is in a container that can contract or expand at constant pressure, at what temperature will the N2 occupy 4.80 L?

Accepted Answer

A) 10°C 
B) 40°C 
C) 146°C 
D) 313°C 
E) 685°C 
A) 10°C 
B) 40°C 
C) 146°C 
D) 313°C 
E) 685°C

Question 4

What is the pressure of the sample of gas trapped in the closed-tube mercury manometer shown below if atmospheric pressure is 751 mmHg and h = 17.3 cm?

Accepted Answer

173 mmHg (

Question 5

Ammonium nitrite undergoes decomposition to produce only gases as shown below.
NH4NO2(s)$\rarr$ N2(g)+ 2H2O(g)
How many liters of gas will be produced by the decomposition of 32.0 g of NH4NO2 at 525°C and 1.5 atm?

Accepted Answer

The answer of Ammonium nitrite undergoes decomposition to produce only...

Question 6

A particular coal sample contains 2.32% S. When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume of SO2(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 * 106 lb of this coal? (1 lb = 454 g)

Accepted Answer

1.6 * 10<s

Question 7

Calculate the volume of H2(g)at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.

Accepted Answer

A) 0.56 L 
B) 1.12 L 
C) 2.23 L 
D) 4.47 L 
E) 3.54 L 
A) 0.56 L 
B) 1.12 L 
C) 2.23 L 
D) 4.47 L 
E) 3.54 L

Question 8

Many automobiles produce about 5 grams of NO for each mile they are driven. How many liters of NO gas at STP would be produced on a 100-mile trip?

Accepted Answer

The answer of Many automobiles produce about 5 grams of...

Question 9

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of hexane (C6H14, density = 0.660 g/mL)completely, yielding carbon dioxide and water?

Accepted Answer

A) 187 L 
B) 712 L 
C) 1780 L 
D) 894 L 
E) 8490 
A) 187 L 
B) 712 L 
C) 1780 L 
D) 894 L 
E) 8490

Question 10

A spacecraft is filled with 0.500 atm of O2 and 0.500 atm of He. If there is a very small hole in the side of this craft such that gas is lost slowly into outer space,

Accepted Answer

A) He is lost 2.8 times faster than O2 is lost. 
B) He is lost 8 times faster than O2 is lost. 
C) He is lost twice as fast as O2 is lost. 
D) O2 is lost 2.8 times faster than He is lost. 
E) O2 is lost 8 times faster than He is lost. 
A) He is lost 2.8 times faster than O2 is lost. 
B) He is lost 8 times faster than O2 is lost. 
C) He is lost twice as fast as O2 is lost. 
D) O2 is lost 2.8 times faster than He is lost. 
E) O2 is lost 8 times faster than He is lost.

Question 11

Give five examples of elements that occur as gases at room temperature and pressure?

Accepted Answer

(Answers will vary.)

Question 12

Calculate the density of N2O gas, in grams per liter, at 110°C and 12 atm.

Accepted Answer

Question 13

Gasoline (which can be considered to be octane, C8H18)burns in oxygen to produce carbon dioxide and water. What volume of carbon dioxide at STP is generated as a result of the combustion of 1.0 gal of gasoline?
(The density of gasoline is 0.81 g/mL. 1 gal = 3.78 L)

Accepted Answer

Question 14

Baking powder is made up of sodium hydrogen carbonate and calcium hydrogen phosphate. When baking powder is wet, these components react to produce carbon dioxide. The equation for this reaction is given below.
NaHCO3(aq)+ CaHPO4(aq)$\rarr$NaCaPO4(aq)+ CO2(g)+ H2O(l)
Assuming all of the carbon dioxide was released as a gas, how many liters of CO2(g)would be formed at room temperature from 4.00 g of NaHCO3 and excess CaHPO4?

Accepted Answer

Approximat

Question 15

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of octane (C8H18, density = 0.7025 g/mL)completely, yielding carbon dioxide and water?

Accepted Answer

A) 718 L 
B) 367 L 
C) 8980 L 
D) 1880 L 
E) 150 L 
A) 718 L 
B) 367 L 
C) 8980 L 
D) 1880 L 
E) 150 L

Question 16

A 1.2 L flask contains 0.500 mole of ammonia (NH3)at 150°C. Calculate the pressure of the ammonia inside the flask.

Accepted Answer

A) 6.91 * 10 -2 atm 
B) 5.13 atm 
C) 12.2 atm 
D) 14.5 atm 
E) 22.4 atm 
A) 6.91 * 10 -2 atm 
B) 5.13 atm 
C) 12.2 atm 
D) 14.5 atm 
E) 22.4 atm

Question 17

Calculate the density of Ar(g)at -11°C and 675 mmHg.

Accepted Answer

A) 1.52 g/L 
B) 1.65 g/L 
C) -39.3 g/L 
D) 39.95 g/L 
E) 1254 g/L 
A) 1.52 g/L 
B) 1.65 g/L 
C) -39.3 g/L 
D) 39.95 g/L 
E) 1254 g/L

Question 18

Samples of the following volatile liquids are opened simultaneously at one end of a room. If you are standing at the opposite end of this room, which species would you smell first? (Assume that your nose is equally sensitive to all these species.)

Accepted Answer

A) ethyl acetate (CH3COOC2H5) 
B) camphor (C10H16O) 
C) diethyl ether (C2H5OC2H5) 
D) naphthalene (C10H8) 
E) pentanethiol (C5H11SH) 
A) ethyl acetate (CH3COOC2H5) 
B) camphor (C10H16O) 
C) diethyl ether (C2H5OC2H5) 
D) naphthalene (C10H8) 
E) pentanethiol (C5H11SH)

Question 19

Give five examples of compounds that exist as gases at room temperature and pressure.

Accepted Answer

(Answers will vary.)

Question 20

What will happen to the height (h)of the mercury column in the manometer shown below if the stopcock is opened, given that the atmospheric pressure is 755 mmHg?

Accepted Answer

A) h will decrease 
B) h will not change 
C) h will increase 
D) not enough information given to answer the question 
A) h will decrease 
B) h will not change 
C) h will increase 
D) not enough information given to answer the question

Exam 5: Gases

Which one of these gases is "lighter-than-air"?

On a spring morning (20°C)you fill your tires to a pressure of 2.25 atmospheres. As you ride along, the tire heats up to 45°C from the friction on the road. What is the pressure in your tires now?

A sample of N2 gas occupies 2.40 L at 20°C. If the gas is in a container that can contract or expand at constant pressure, at what temperature will the N2 occupy 4.80 L?

What is the pressure of the sample of gas trapped in the closed-tube mercury manometer shown below if atmospheric pressure is 751 mmHg and h = 17.3 cm?

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH4NO2(s) →\rarr→ N2(g)+ 2H2O(g) How many liters of gas will be produced by the decomposition of 32.0 g of NH4NO2 at 525°C and 1.5 atm?

A particular coal sample contains 2.32% S. When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume of SO2(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 * 106 lb of this coal? (1 lb = 454 g)

Calculate the volume of H2(g)at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.

Many automobiles produce about 5 grams of NO for each mile they are driven. How many liters of NO gas at STP would be produced on a 100-mile trip?

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of hexane (C6H14, density = 0.660 g/mL)completely, yielding carbon dioxide and water?

A spacecraft is filled with 0.500 atm of O2 and 0.500 atm of He. If there is a very small hole in the side of this craft such that gas is lost slowly into outer space,

Give five examples of elements that occur as gases at room temperature and pressure?

Calculate the density of N2O gas, in grams per liter, at 110°C and 12 atm.

Gasoline (which can be considered to be octane, C8H18)burns in oxygen to produce carbon dioxide and water. What volume of carbon dioxide at STP is generated as a result of the combustion of 1.0 gal of gasoline? (The density of gasoline is 0.81 g/mL. 1 gal = 3.78 L)

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of octane (C8H18, density = 0.7025 g/mL)completely, yielding carbon dioxide and water?

A 1.2 L flask contains 0.500 mole of ammonia (NH3)at 150°C. Calculate the pressure of the ammonia inside the flask.

Calculate the density of Ar(g)at -11°C and 675 mmHg.

Samples of the following volatile liquids are opened simultaneously at one end of a room. If you are standing at the opposite end of this room, which species would you smell first? (Assume that your nose is equally sensitive to all these species.)

Give five examples of compounds that exist as gases at room temperature and pressure.

What will happen to the height (h)of the mercury column in the manometer shown below if the stopcock is opened, given that the atmospheric pressure is 755 mmHg?

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

A sample of N₂ gas occupies 2.40 L at 20°C. If the gas is in a container that can contract or expand at constant pressure, at what temperature will the N₂ occupy 4.80 L?

Ammonium nitrite undergoes decomposition to produce only gases as shown below. NH₄NO₂(s) $\rarr$ N₂(g)+ 2H₂O(g) How many liters of gas will be produced by the decomposition of 32.0 g of NH₄NO₂ at 525°C and 1.5 atm?

A particular coal sample contains 2.32% S. When the coal is burned, the sulfur is converted to sulfur dioxide gas. What volume of SO₂(g), measured at 25°C and 749 mmHg, is produced by burning 2.0 * 10⁶ lb of this coal? (1 lb = 454 g)

Calculate the volume of H₂(g)at 273 K and 2.00 atm that will be formed when 275 mL of 0.725 M HCl solution reacts with excess Mg to give hydrogen gas and aqueous magnesium chloride.

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of hexane (C₆H₁₄, density = 0.660 g/mL)completely, yielding carbon dioxide and water?

A spacecraft is filled with 0.500 atm of O₂ and 0.500 atm of He. If there is a very small hole in the side of this craft such that gas is lost slowly into outer space,

Calculate the density of N₂O gas, in grams per liter, at 110°C and 12 atm.

Gasoline (which can be considered to be octane, C₈H₁₈)burns in oxygen to produce carbon dioxide and water. What volume of carbon dioxide at STP is generated as a result of the combustion of 1.0 gal of gasoline? (The density of gasoline is 0.81 g/mL. 1 gal = 3.78 L)

The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of octane (C₈H₁₈, density = 0.7025 g/mL)completely, yielding carbon dioxide and water?

A 1.2 L flask contains 0.500 mole of ammonia (NH₃)at 150°C. Calculate the pressure of the ammonia inside the flask.