Question 1

What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 736 mmHg and h = 9.2 cm?

Accepted Answer

A) 92 mmHg 
B) 644 mmHg 
C) 736 mmHg 
D) 828 mmHg 
A) 92 mmHg 
B) 644 mmHg 
C) 736 mmHg 
D) 828 mmHg

Question 2

What is the pressure (in atmospheres)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 735 mmHg and h = 8.3 cm?

Accepted Answer

The answer of What is the pressure (in atmospheres)of the...

Question 3

A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0 atm, to the water's surface, where the temperature is 25°C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.

Accepted Answer

A) 0.72 mL 
B) 6.2 mL 
C) 41.4 mL 
D) 22.4 mL 
E) 7.1 mL 
A) 0.72 mL 
B) 6.2 mL 
C) 41.4 mL 
D) 22.4 mL 
E) 7.1 mL

Question 4

The van der Waals equation is a modification of the ideal gas equation. For what two facts does this equation account?

Accepted Answer

(1)Real gas molecule

Question 5

A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28°C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28°C is 28.3 mmHg.

Accepted Answer

A) 5.0 * 1022 
B) 5.2 * 1022 
C) 3.8 * 1023 
D) 5.4 * 1023 
E) 3.8 F* 1025 
A) 5.0 * 1022 
B) 5.2 * 1022 
C) 3.8 * 1023 
D) 5.4 * 1023 
E) 3.8 F* 1025

Question 6

What is V in the table below?

Accepted Answer

The answer of What is V in the table below?...

Question 7

A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35°C and 678 mmHg. Identify the Noble gas in this sample? (R = 0.08206 L.atm/K.mol)

Accepted Answer

A) He 
B) Ne 
C) Ar 
D) Kr 
E) Xe 
A) He 
B) Ne 
C) Ar 
D) Kr 
E) Xe

Question 8

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C. Which of these choices is its molecular formula?

Accepted Answer

A) NO 
B) NO2 
C) N3O6 
D) N2O4 
E) N2O5 
A) NO 
B) NO2 
C) N3O6 
D) N2O4 
E) N2O5

Question 9

What is standard temperature and standard pressure?

Accepted Answer

0°C and 1

Question 10

How many molecules of N2 gas can be present in a 2.5 L flask at 50°C and 650 mmHg?

Accepted Answer

A) 2.1 * 10 -23 molecules 
B) 4.9 * 1022 molecules 
C) 3.1 * 1023 molecules 
D) 3.6 * 1025 molecules 
E) 0.081 molecules 
A) 2.1 * 10 -23 molecules 
B) 4.9 * 1022 molecules 
C) 3.1 * 1023 molecules 
D) 3.6 * 1025 molecules 
E) 0.081 molecules

Question 11

A sample of mercury(II)oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25°C. One now finds that the gas pressure inside the container is 1.73 atm. What mass of mercury(II)oxide was originally placed into the container?

Accepted Answer

A) 913 g 
B) 76.6 g 
C) 1.51 g 
D) 45.6 g 
E) 153 g 
A) 913 g 
B) 76.6 g 
C) 1.51 g 
D) 45.6 g 
E) 153 g

Question 12

At constant pressure, the density of a gas depends on temperature. Does the density increase or decrease as the temperature increases?

Accepted Answer

The answer of At constant pressure, the density of a...

Question 13

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO2 and is heated to 400°C, will it burst?

Accepted Answer

Question 14

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?

Accepted Answer

A) 0.258 atm 
B) 301 mmHg 
C) 356 mmHg 
D) 5,345 mmHg 
E) 8,020 mmHg 
A) 0.258 atm 
B) 301 mmHg 
C) 356 mmHg 
D) 5,345 mmHg 
E) 8,020 mmHg

Question 15

A 0.271 g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg. The empirical formula of the compound is CH2. What is the molecular formula of the compound?

Accepted Answer

A) CH2 
B) C2H4 
C) C3H6 
D) C4H8 
E) C6H12 
A) CH2 
B) C2H4 
C) C3H6 
D) C4H8 
E) C6H12

Question 16

The pressure of a gas sample was measured to be 489 mmHg. Which of the following is not an equivalent statement of that pressure? (1 atm = 1.01325 * 105 Pa)

Accepted Answer

A) 65.2 kPa 
B) 6.52 * 104 Pa 
C) 489 torr 
D) 0.811 atm 
A) 65.2 kPa 
B) 6.52 * 104 Pa 
C) 489 torr 
D) 0.811 atm

Question 17

Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25°C. R = 0.08206 L.atm/K.mol.

Accepted Answer

A) 0.060 L 
B) 1.34 L 
C) 16.9 L 
D) 24.2 L 
E) 734 L 
A) 0.060 L 
B) 1.34 L 
C) 16.9 L 
D) 24.2 L 
E) 734 L

Question 18

Calculate the number of moles of gas contained in a 10.0 L tank at 22°C and 105 atm. (R = 0.08206 L.atm/K.mol)

Accepted Answer

A) 1.71 * 10-3 mol 
B) 0.0231 mol 
C) 1.03 mol 
D) 43.4 mol 
E) 582 mol 
A) 1.71 * 10-3 mol 
B) 0.0231 mol 
C) 1.03 mol 
D) 43.4 mol 
E) 582 mol

Question 19

A sample of a gas occupies 1.40 * 103 mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

Accepted Answer

A) 2,800 mL 
B) 2,100 mL 
C) 1,400 mL 
D) 1,050 mL 
E) 700 mL 
A) 2,800 mL 
B) 2,100 mL 
C) 1,400 mL 
D) 1,050 mL 
E) 700 mL

Question 20

Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O2)when stored at 22°C in a 40.0 L cylinder?

Accepted Answer

A) 3.55 atm 
B) 1,510 atm 
C) 47.3 atm 
D) 7.56 *104 atm 
E) 10.2 atm 
A) 3.55 atm 
B) 1,510 atm 
C) 47.3 atm 
D) 7.56 *104 atm 
E) 10.2 atm

Exam 5: Gases

What is the pressure of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 736 mmHg and h = 9.2 cm?

What is the pressure (in atmospheres)of the sample of gas trapped in the open-tube mercury manometer shown below if atmospheric pressure is 735 mmHg and h = 8.3 cm?

A small bubble rises from the bottom of a lake, where the temperature and pressure are 4°C and 3.0 atm, to the water's surface, where the temperature is 25°C and the pressure is 0.95 atm. Calculate the final volume of the bubble if its initial volume was 2.1 mL.

The van der Waals equation is a modification of the ideal gas equation. For what two facts does this equation account?

A sample of carbon monoxide gas was collected in a 2.0 L flask by displacing water at 28°C and 810 mmHg. Calculate the number of CO molecules in the flask. The vapor pressure of water at 28°C is 28.3 mmHg.

What is V in the table below?

A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35°C and 678 mmHg. Identify the Noble gas in this sample? (R = 0.08206 L.atm/K.mol)

A gaseous compound is 30.4% nitrogen and 69.6% oxygen by mass. A 5.25-g sample of the gas occupies a volume of 1.00 L and exerts a pressure of 1.26 atm at -4.0°C. Which of these choices is its molecular formula?

What is standard temperature and standard pressure?

How many molecules of N2 gas can be present in a 2.5 L flask at 50°C and 650 mmHg?

At constant pressure, the density of a gas depends on temperature. Does the density increase or decrease as the temperature increases?

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO2 and is heated to 400°C, will it burst?

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?

A 0.271 g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg. The empirical formula of the compound is CH2. What is the molecular formula of the compound?

The pressure of a gas sample was measured to be 489 mmHg. Which of the following is not an equivalent statement of that pressure? (1 atm = 1.01325 * 105 Pa)

Calculate the volume occupied by 25.2 g of CO2 at 0.84 atm and 25°C. R = 0.08206 L.atm/K.mol.

Calculate the number of moles of gas contained in a 10.0 L tank at 22°C and 105 atm. (R = 0.08206 L.atm/K.mol)

A sample of a gas occupies 1.40 * 103 mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O2)when stored at 22°C in a 40.0 L cylinder?

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

How many molecules of N₂ gas can be present in a 2.5 L flask at 50°C and 650 mmHg?

An aerosol can with a volume of 0.50 L has a bursting point of 2.6 atm. If the can contains 1.0 g CO₂ and is heated to 400°C, will it burst?

A mixture of three gases has a total pressure of 1,380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO₂, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?

A 0.271 g sample of an unknown vapor occupies 294 mL at 140°C and 847 mmHg. The empirical formula of the compound is CH₂. What is the molecular formula of the compound?

The pressure of a gas sample was measured to be 489 mmHg. Which of the following is not an equivalent statement of that pressure? (1 atm = 1.01325 * 10⁵ Pa)

Calculate the volume occupied by 25.2 g of CO₂ at 0.84 atm and 25°C. R = 0.08206 L.atm/K.mol.

A sample of a gas occupies 1.40 * 10³ mL at 25°C and 760 mmHg. What volume will it occupy at the same temperature and 380 mmHg?

Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be exerted by 2,500 g of oxygen gas (O₂)when stored at 22°C in a 40.0 L cylinder?