7. Gases

The Ideal Gas Law Derivations

Ideal Gas Law: Where did R come from?

Assume that you have a cylinder with a movable piston. What
would happen to the gas pressure inside the cylinder if you
were to do the following?
(c) Decrease the volume by 45% at constant T

Many gases are shipped in high-pressure containers. Consider
a steel tank whose volume is 210.0 L that contains O2
gas at a pressure of 16,500 kPa at 23 °C. (c) At what temperature would the pressure in the tank equal 15.2 MPa?

Consider the apparatus shown in the following drawing.
(a) When the valve between the two containers is opened
and the gases are allowed to mix, what is the partial pressure of N2
after mixing?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/84f8d38d88c5e562-1664296088311.jpg" alt="" />

A balloon contains 0.158 mol of gas and has a volume of 2.46 L.
If an additional 0.113 mol of gas is added to the balloon (at the
same temperature and pressure), what is its final volume?

An ideal gas at a pressure of 152 kPa is contained in a bulb
of unknown volume. A stopcock is used to connect this
bulb with a previously evacuated bulb that has a volume
of 0.800 L as shown here. When the stopcock is opened,
the gas expands into the empty bulb. If the temperature
is held constant during this process and the final pressure
is 92.66 kPa, what is the volume of the bulb that was
originally filled with gas?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/4ec1c998ae0f3b08-1660668304012.jpg" alt="" />

A sample of gas has an initial volume of 5.6 L at a pressure of
735 mmHg. If the volume of the gas is increased to 9.4 L, what
is its pressure?

A syringe containing 1.55 mL of oxygen gas is cooled from
95.3 °C to 0.0 °C. What is the final volume of oxygen gas?

The Ideal Gas Law Derivations Example 1

Ideal Gas Law (PV=nRT) Derivation from Boyle's Law, Charles Law and Avogadro's Law

Ideal Gas Law | General Gas Equation | Chemistry

Be Lazy! Don't Memorize the Gas Laws!

Kinetic Molecular Theory and the Ideal Gas Laws

A cylinder with a moveable piston contains 0.553 mol of gas
and has a volume of 253 mL. What is its volume if an additional
0.365 mol of gas is added to the cylinder? (Assume constant
temperature and pressure.)

A sample of nitrogen gas in a 1.75-L container exerts a pressure
of 1.35 atm at 25 °C. What is the pressure if the volume of the
container is maintained constant and the temperature is raised
to 355 °C?

Assume that you have a cylinder with a movable piston. What
would happen to the gas pressure inside the cylinder if you
were to do the following?
(a) Triple the Kelvin temperature while holding the volume
constant

(b) If a car tire is filled to a pressure of 220.6 kPa measured at 24 °C,
what will be the tire pressure if the tires heat up to 49 °C
during driving?

The Ideal Gas Law: Crash Course Chemistry #12

A 48.3-mL sample of gas in a cylinder is warmed from 22 °C to
87 °C. What is its volume at the final temperature?

Ideal Gas Law :PV=nRT | Kinetic Theory | Ideal Gas Equation class 11 Chemistry | Thermodynamics

Assume that you have a cylinder with a movable piston. 
What would happen to the gas volume of the cylinder if you 
were to do the following? 
(a) Halve the Kelvin temperature while holding the pressure 
constant

Gas density and PV=nRT, the ideal gas law

How to derive the ideal gas equation -Equation for ideal gas (PV=nRT) - PV =nRT derivation - Kisembo

Consider a lake that is about 40 m deep. A gas bubble with a
diameter of 1.0 mm originates at the bottom of a lake where
the pressure is 405.3 kPa. Calculate its volume when the bubble
reaches the surface of the lake where the pressure is 98
kPa, assuming that the temperature does not change.

A sample of nitrogen dioxide gas at 130 ºC and 315 torr occupies a volume of 500 mL. What will the gas pressure be if the volume is reduced to 320 mL at 130 ºC?

Aerosol cans carry clear warnings against incineration because
of the high pressures that can develop upon heating. Suppose
that a can contains a residual amount of gas at a pressure of
755 mmHg and a temperature of 25 °C. What would the pressure
be if the can were heated to 1155 °C?

Assume that you have a cylinder with a movable piston. 
What would happen to the gas volume of the cylinder if you 
were to do the following? 
(b) Increase the amount of gas by one-fourth while holding 
the temperature and pressure constant

A cylinder with a movable piston contains 0.615 moles of gas and has a volume of 295 mL. What will its volume be if 0.103 moles of gas escaped?

On most spray cans it is advised to never expose them to fire. A spray can is used until all that remains is the propellant gas, which has a pressure of 1350 torr at 25 ºC. If the can is then thrown into a fire at 455 ºC, what will be the pressure (in torr) in the can?a) 750 torrb) 1800 torrc) 2190 torrd) 2850 torre) 3300 torr

Ideal Gas Law Introduction

Imagine that the reaction 2 CO1g2 + O21g2¡2 CO21g2
occurs in a container that has a piston that moves to maintain
a constant pressure when the reaction occurs at constant temperature.
Which of the following statements describes how the
volume of the container changes due to the reaction: (a) the
volume increases by 50%, (b) the volume increases by 33%,
(c) the volume remains constant, (d) the volume decreases by
33%, (e) the volume decreases by 50%.

A sample of gas has an initial volume of 13.9 L at a pressure of
1.22 atm. If the sample is compressed to a volume of 10.3 L,
what is its pressure?

A small cylinder of helium gas used for filling balloons has 
a volume of 2.30 L and a pressure of 13,800 kPa at 25 °C. 
How many balloons can you fill if each one has a volume of 
1.5 L and a pressure of 1.25 atm at 25 °C?

A scuba diver creates a spherical bubble with a radius of 2.5 cm
at a depth of 30.0 m where the total pressure (including
atmospheric pressure) is 4.00 atm. What is the radius of the
bubble when it reaches the surface of the water? (Assume that
the atmospheric pressure is 1.00 atm and the temperature is
298 K.)

Consider the arrangement of bulbs shown in the drawing.
Each of the bulbs contains a gas at the pressure shown.
What is the pressure of the system when all the stopcocks
are opened, assuming that the temperature remains constant?
(We can neglect the volume of the capillary tubing
connecting the bulbs.)<img src="https://lightcat-files.s3.amazonaws.com/problem_images/af75aacc5991e7d5-1660667069453.jpg" alt="" />

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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&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.

The Ideal Gas Law: Density

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;