Question 1

What is P in the table below?

Accepted Answer

2 atm

Question 2

How many grams of N2O, nitrous oxide, are contained in 500.mL of the gas at STP?

Accepted Answer

0.982 g

Question 3

The temperature of an ideal gas in a 5.00 L container originally at 1 atm pressure and 25°C is lowered to 220 K. Calculate the new pressure of the gas.

Accepted Answer

A) 1.0 atm 
B) 1.35 atm 
C) 8.8 atm 
D) 0.738 atm 
E) 0.114 atm 
A) 1.0 atm 
B) 1.35 atm 
C) 8.8 atm 
D) 0.738 atm 
E) 0.114 atm D

Question 4

The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

Accepted Answer

A) pressure. 
B) temperature. 
C) volume. 
D) density. 
A) pressure. 
B) temperature. 
C) volume. 
D) density.

Question 5

Determine the molar mass of chloroform gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm3 at 97°C. The pressure of the chloroform is 728 mmHg.

Accepted Answer

A) 187 g/mol 
B) 121 g/mol 
C) 112 g/mol 
D) 31.6 g/mol 
E) 8.28 * 10-3 g/mol 
A) 187 g/mol 
B) 121 g/mol 
C) 112 g/mol 
D) 31.6 g/mol 
E) 8.28 * 10-3 g/mol

Question 6

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 7

A block of dry ice (solid CO2, density = 1.56 g/mL)of dimensions 25.0 cm * 25.0 cm * 25.0 cm is left to sublime (i.e.to pass from the solid phase to the gas phase)in a closed chamber of dimensions 4.00 m * 5.00 m *3.00 m. The partial pressure of carbon dioxide in this chamber at 25°C will be

Accepted Answer

A) 171 mmHg 
B) 107 mmHg 
C) 0.225 mmHg 
D) 0.171 mmHg 
E) 14.4 mmHg 
A) 171 mmHg 
B) 107 mmHg 
C) 0.225 mmHg 
D) 0.171 mmHg 
E) 14.4 mmHg

Question 8

Calculate the density, in g/L, of SF6 gas at 27°C and 0.500 atm pressure.

Accepted Answer

A) 3.38 * 10-3 g/L 
B) 2.96 g/L 
C) 22.4 g/L 
D) 32.9 g/L 
E) 3.38 kg/L 
A) 3.38 * 10-3 g/L 
B) 2.96 g/L 
C) 22.4 g/L 
D) 32.9 g/L 
E) 3.38 kg/L

Question 9

What is the pressure (in atmospheres)of the sample of gas trapped in the closed-tube mercury manometer shown below if h = 23.6 cm?

Accepted Answer

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

Question 10

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 11

The pressure of a gas sample was measured to be 654 mmHg.What is the pressure in kPa? (1 atm = 1.01325 * 105 Pa)

Accepted Answer

A) 87.2 kPa 
B) 118 kPa 
C) 6.63 * 104 kPa 
D) 8.72 * 104 kPa 
E) 8.72 * 107 kPa 
A) 87.2 kPa 
B) 118 kPa 
C) 6.63 * 104 kPa 
D) 8.72 * 104 kPa 
E) 8.72 * 107 kPa

Question 12

At STP, 1 mole of gas has a molar volume of 22.4 L.What is the density of oxygen at STP?

Accepted Answer

The answer of At STP, 1 mole of gas has...

Question 13

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 14

What is the definition of a "gas"?

Accepted Answer

A "gas" is a substance in whic

Question 15

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 16

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 17

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 18

At what temperature will a fixed amount of gas with a volume of 175 L at 15°C and 760 mmHg occupy a volume of 198 L at a pressure of 640 mm Hg?

Accepted Answer

A) 274°C 
B) 214°C 
C) 114°C 
D) 1°C 
E) -59°C 
A) 274°C 
B) 214°C 
C) 114°C 
D) 1°C 
E) -59°C

Question 19

If 30.0 L of oxygen are cooled from 200ºC to 1°C at constant pressure, what is the new volume of oxygen?

Accepted Answer

A) 0.150 L 
B) 17.4 L 
C) 23.0 L 
D) 51.8 L 
E) 6.00 * 103 L 
A) 0.150 L 
B) 17.4 L 
C) 23.0 L 
D) 51.8 L 
E) 6.00 * 103 L

Question 20

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 (

Exam 5: Gases

What is P in the table below?

How many grams of N2O, nitrous oxide, are contained in 500.mL of the gas at STP?

The temperature of an ideal gas in a 5.00 L container originally at 1 atm pressure and 25°C is lowered to 220 K. Calculate the new pressure of the gas.

The molecules of different samples of an ideal gas have the same average kinetic energies, at the same

Determine the molar mass of chloroform gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm3 at 97°C. The pressure of the chloroform is 728 mmHg.

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)

A block of dry ice (solid CO2, density = 1.56 g/mL)of dimensions 25.0 cm * 25.0 cm * 25.0 cm is left to sublime (i.e.to pass from the solid phase to the gas phase)in a closed chamber of dimensions 4.00 m * 5.00 m *3.00 m. The partial pressure of carbon dioxide in this chamber at 25°C will be

Calculate the density, in g/L, of SF6 gas at 27°C and 0.500 atm pressure.

What is the pressure (in atmospheres)of the sample of gas trapped in the closed-tube mercury manometer shown below if h = 23.6 cm?

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 pressure of a gas sample was measured to be 654 mmHg.What is the pressure in kPa? (1 atm = 1.01325 * 105 Pa)

At STP, 1 mole of gas has a molar volume of 22.4 L.What is the density of oxygen at STP?

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

What is the definition of a "gas"?

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?

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?

At what temperature will a fixed amount of gas with a volume of 175 L at 15°C and 760 mmHg occupy a volume of 198 L at a pressure of 640 mm Hg?

If 30.0 L of oxygen are cooled from 200ºC to 1°C at constant pressure, what is the new volume of oxygen?

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?

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Thermo-Chemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

Entropy, Free Energy, and Equilibrium

Electrochemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metal Chemistry and Coordination Compounds

Nuclear Chemistry

Organic Chemistry

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Filters

How many grams of N₂O, nitrous oxide, are contained in 500.mL of the gas at STP?

Determine the molar mass of chloroform gas if a sample weighing 0.389 g is collected in a flask with a volume of 102 cm³ at 97°C. The pressure of the chloroform is 728 mmHg.

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)

A block of dry ice (solid CO₂, density = 1.56 g/mL)of dimensions 25.0 cm * 25.0 cm * 25.0 cm is left to sublime (i.e.to pass from the solid phase to the gas phase)in a closed chamber of dimensions 4.00 m * 5.00 m *3.00 m. The partial pressure of carbon dioxide in this chamber at 25°C will be

Calculate the density, in g/L, of SF₆ gas at 27°C and 0.500 atm pressure.

The pressure of a gas sample was measured to be 654 mmHg.What is the pressure in kPa? (1 atm = 1.01325 * 10⁵ Pa)

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?