7. Gases

The Ideal Gas Law: Density

Molar Mass and Density Using Ideal Gas Law

What is the density in g/L of a gas mixture that contains 27.0% 
F2 and 73.0% He by volume at 714 mm Hg and 27.5 °C?

The Ideal Gas Law: Density Example 2

(a) Calculate the density of dinitrogen tetroxide gas 1N2O42
at 111.5 kPa and 0 °C.

Rank the following gases and vapors from least dense
to most dense at 101.33 kPa and 298 K: water vapor
1H2O1g22, nitrogen 1N22, hydrogen sulfide 1H2S2.

Propane, C3H8, liquefies under modest pressure, allowing a
large amount to be stored in a container.
(a) Calculate the number of moles of propane gas in a 20-L container at 709.3 kPa and 25 C. 
(b) Calculate the number of moles of liquid propane that can be stored in the same volume if the density of the liquid is 0.590 g/mL. 
(c) Calculate the ratio of the number of moles of liquid to moles of gas. Discuss this ratio in light of the kinetic-molecular theory of gases.

A 1.0-L container of liquid nitrogen is kept in a closet measuring
1.0 m by 1.0 m by 2.0 m. Assuming that the container is completely
full, that the temperature is 25.0 °C, and that the atmospheric
pressure is 1.0 atm, calculate the percent (by volume) of
air that is displaced if all of the liquid nitrogen evaporates. (Liquid
nitrogen has a density of 0.807 g/mL.)

(b) Calculate the molar mass of a vapor that
has a density of 7.135 g>L at 12 °C and 99.06 kPa.

Consider the following samples of gases:
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/fd8bdda34304dd25-1664296385364.jpg" alt="" />
If the three samples are all at the same temperature, rank
them with respect to (c) density

Consider two containers of gases at the same temperature. One has helium at a pressure of 1.00 atm. The other contains carbon dioxide with the same density as the helium gas. What is the pressure of the carbon dioxide gas sample?

Determine the molecular formula of a gaseous compound that is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen. At 27°C, the density of the gas is 1.5535 g/L and it exerts a pressure of 0.092 atm.

What are the molecular weights of the gases with the following
densities:
(b) 1.053 g/L at 25 °C and 752 mm Hg

A sample of N2O gas has a density of 2.85 g/L at 298 K. What is
the pressure of the gas (in mmHg)?

Rank the following gases from least dense to most dense at
101.33 kPa and 298 K: O2, Ar, NH3, HCl.

Gas density and PV=nRT, the ideal gas law

An 11.5-mL sample of liquid butane (density = 0.573 g>mL) is
evaporated in an otherwise empty container at a temperature of
28.5 °C. The pressure in the container following evaporation is
892 torr. What is the volume of the container?

A gas mixture composed of helium and argon has a density of
0.670 g>L at a 755 mmHg and 298 K. What is the composition
of the mixture by volume?

The matter in interstellar space consists almost entirely of hydrogen atoms at a temperature of 100 K and a density of approximately 1 atom>cm3. What is the gas pressure in millimeters of mercury?

What is the density (in g/L) of hydrogen gas at 20.0 °C and a
pressure of 1655 psi?

Two 112-L tanks are filled with gas at 330 K. One contains 
5.00 mol of Kr, and the other contains 5.00 mol of O2. 
Considering the assumptions of kinetic–molecular theory, 
rank the gases from low to high for each of the following 
properties. 
(b) Density (g/L)

Find the Density of a Gas (Ideal Gas Law)

Using molar mass and density (d), the ideal gas law can be rewritten as: d = (P &#215; Molar Mass)/(RT) where R is the ideal gas constant.

Remember that n = mass/(Molar Mass), and density = mass/volume. Substitute into the ideal gas law to solve for density.

Calculate the density of argon gas at 22.5&#x2103; and a pressure of 2.0 atm.

The density of a gas of unknown molar mass was
measured as a function of pressure at 0 C, as in the table
that follows. (a) Determine a precise molar mass for the
gas. [Hint: Graph d>P versus P.] 
<TABLE>

The density of a gas of unknown molar mass was
measured as a function of pressure at 0 C, as in the table
that follows. (b) Why is d>P not a constant as a function of pressure?
<TABLE><img src="https://lightcat-files.s3.amazonaws.com/problem_images/1c740f25e1431ca4-1660742796590.jpg" alt="" />

The Ideal Gas Law and Molar Mass and Density of a Gas

A quantity of N2 occupies a volume of 1.0 L at 300 K and 1.0 atm.
The gas expands to a volume of 3.0 L as the result of a change in
both temperature and pressure. Find the density of the gas at
these new conditions.

The Ideal Gas Law: Density Example 1

Applications of the Ideal Gas Law:  Density of a Gas

Using the Ideal Gas Law to Determine the Density of a Gas

Learn the toughest concepts covered in Chemistry with step-by-step video tutorials and practice problems by world-class tutors

Jules

General Chemistry

https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/general-chemistry

#FFFFFF

Crash Chemistry Academy

Pathways to Chemistry

Ben's Chem Videos

BoylanChemistry

Chemin10

chemistNATE

Jules Bruno

1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Partial Pressure

Partial Pressure (PGas) is the pressure exerted by an individual gas within a container.

Velocity Distributions

Velocity Distributions represent probability distributions for a gas when examining their molar mass and temperature.

Mole Fraction

Mole Fraction (X) represents the mole component by total moles.&nbsp;

Mole Fraction -

The Ideal Gas Law Derivations

The&nbsp;Ideal Gas Law Derivations are a convenient way to solve gas calculations involving 2 sets of the same variables.&nbsp;

Root Mean Square Speed

Root Mean Square Speed&nbsp;allows for the determination of the velocity of 1 type of gas molecule.

Under certain conditions of pressure and temperature, the Ideal Gas Law can determine the density&nbsp;of a gas.&nbsp;

Effusion

Effusion is the escaping of gas molecules or atoms through a pinhole.&nbsp;

Kinetic Energy of Gases

Kinetic Energy is the energy an object possesses due to its motion.

Gas Stoichiometry

Gas Stoichiometry involves chemical reactions that contain gases.

The Ideal Gas Law

The Ideal Gas Law formula relates the behavior of gases under varying conditions of pressure, volume, moles and temperature.

Chemistry Gas Laws: Combined Gas Law

The Combined Gas Law&nbsp;is created from “combining” Boyle’s Law, Charles’ Law, and Gay–Lussac’s Law.

Pressure Units

Pressure is the force that is exerted within a given volume of space.&nbsp;

Kinetic Molecular Theory

A gas is seen as a collection of molecules or individual atoms that are in constant motion. The Kinetic-Molecular Theory tries to use data of real gases to predict how an ideal gas would behave if they existed.&nbsp;&nbsp;

Standard Temperature and Pressure

In order to accurately study the effect that changes in pressure, temperature and moles have on volume, chemists will often run their experiments under Standard Temperature and Pressure.&nbsp;

The Ideal Gas Law Applications

The Ideal Gas Law Applications establish both the direct and inverse relationships between the Ideal Gas Law variables.

Maxwell-Boltzmann Distribution

The Maxwell-Boltzmann Distribution is a probability distribution curve that describes the speed of a gas at a specific temperature.

Chemistry Gas Laws

Chemistry Gas Laws&nbsp;are laws that relate together the pressure, volume and temperature of a gas.

The Ideal Gas Law: Molar Mass

The Ideal Gas Law can be further extended to find the molar mass of a gas.&nbsp;

Van der Waals Equation

The&nbsp;Van der Waals Equation is used when dealing with real, non-ideal gases.&nbsp;