7. Gases

Kinetic Energy of Gases

Chemistry of Gases (32 of 40) Kinetic Energy of a Gas Molecule

A 10.0 L flask contains a mixture of neon and argon gases at a pressure of 2.38 atm. Calculate the total kinetic energy of the gaseous mixture.

Calculate the root mean square velocity and kinetic energy of
CO, CO2, and SO3 at 298 K. Which gas has the greatest velocity? The greatest kinetic energy? The greatest effusion rate?

Kinetic Energy of Gases Example 1

You have an evacuated container of fixed volume and
known mass and introduce a known mass of a gas sample.
Measuring the pressure at constant temperature over time,
you are surprised to see it slowly dropping. You measure the
mass of the gas-filled container and find that the mass is
what it should be—gas plus container—and the mass does
not change over time, so you do not have a leak. Suggest an
explanation for your observations.

At 25 °C (approximately room temperature) the rms velocity
of an Ar atom in air is 1553 km>h. (b) What is the kinetic energy (in J) of an Ar atom
moving at this speed?

A baseball with a mass of 503 g possesses a kinetic energy of 0.815 kJ. Calculate its velocity in m/s.

Suppose you have two 1-L flasks, one containing N2 at STP, 
the other containing CH4 at STP. How do these systems compare 
with respect to (c) average kinetic energy of the molecules?

A flask at room temperature contains exactly equal amounts (in 
moles) of nitrogen and xenon. 
c. The molecules of which gas have the greater average kinetic 
energy?

Calculate the kinetic energy of
F2, Cl2, and Br2 at 298 K.

Consider a 1.0-L sample of helium gas and a 1.0-L sample
of argon gas, both at room temperature and atmospheric
pressure.
a. Do the atoms in the helium sample have the same average
kinetic
energy as the atoms in the argon sample?

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[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.

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 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;

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