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# Ideal Gas Law (IGNORE)

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Sections
Pressure Units
The Ideal Gas Law
The Ideal Gas Law Derivations
The Ideal Gas Law Applications
Chemistry Gas Laws
Chemistry Gas Laws: Combined Gas Law
Mole Fraction
Partial Pressure
The Ideal Gas Law: Molar Mass
The Ideal Gas Law: Density
Gas Stoichiometry
Standard Temperature and Pressure
Effusion
Root Mean Square Speed
Kinetic Energy of Gases
Maxwell-Boltzmann Distribution
Velocity Distributions
Kinetic Molecular Theory
Van der Waals Equation
Boyle's Law (IGNORE)
Charles Law (IGNORE)
Ideal Gas Law (IGNORE)
Jules Bruno

The Ideal Gas Law represents a formula that relates the behavior of gases under varying conditions of concentration, volume, pressure and temperature.

The Ideal Gas Law

Within a closed container, gas molecules behave ideally when the temperature and volume are high while the pressure is low. The Ideal Gas Law equation is represented as:

Ideal Gas Law

R Constant (R)

The variable of R represents the universal gas constant of the gas. When atmospheres (atm) are incorporated into its units the traditional R value of 0.08206 is used, but changing atmospheres (atm) will change the numerical value of R.

Universal R Constant (Different Forms)

Pressure (P)

The variable of P represents the pressure of the gas. Although the SI unit for pressure is pascals, it is customary to use the units of atmospheres (atm).

Units of Pressure

1.0 atmosphere (atm) is equal to each of the given pressure units based on the given value. For example, 1.0 atm = 760 torrs or 1.0 atm = 101.325 kPa.

Volume (V)

The variable of V represents the volume of the gas. The units are in Liters.

Temperature (T)

The variable of T represents the absolute temperature of the gas. The units are in Kelvin. Let’s say you are given 90oF and asked to convert it into Kelvin.

Conversion from Fahrenheit to Celsius:

Fahrenheit to Celsius ConversionConversion from Celsius to Kelvin:

Celsius to Kelvin Conversion

Moles (n)

The variable of n represents the moles of the gas.

PRACTICE:

How many grams of neon gas are present in a 5.0 L container at pressure of 1.35 atm at 35oC?

STEP 1: Identify the variables given.

Problem Outline

STEP 2: Isolate the missing variable of moles (n).

Solving for moles (n)

STEP 3: Convert the moles (n) into grams.

Moles to Grams Conversion

Further Applications of the Ideal Gas Law

The Ideal Gas Law can be rearranged in order to create new equations that determine either the density or molar mass of a gas molecule.

When dealing with the density of a gas molecule we can utilize the following equation:

Derived Gas Law (Density)

Pressure, R constant and Temperature

The variables of P, R and T still represent pressure, the gas constant, and temperature in Kelvin.

Molar Mass (M)

The variable of M represents the molar mass of a gas molecule. The units of molar mass are grams per mole (g/mol).

Density (d)

The variable of d represents the density of a gas molecule. As a result of being less dense than solids or liquids, gas molecules have their density in units of grams per liter (g/L).

PRACTICE: Determine the density of NH3 gas at 435 K and 1.00 atm.

STEP 1: Identify the variables given.

Identify given variables

STEP 2: Solve for the missing variable of density (d).

Solving for missing variable (density)

When dealing with the mass and molar mass of a gas molecule we can utilize the following equation:

Derived Gas Law (Molar Mass)

Pressure, Volume, R constant, Molar Mass and Temperature

The variables of P,V, M, R and T are the same ones used from the previous equations.

Mass (m)

The variable of m represents the mass of a gas molecule. The units of mass are grams (g).

PRACTICE: An unknown gas contained in a 1.85 L flask is weighed and found to have a mass of 15.87 g at a pressure of 2.45 atm and a temperature of 18.6°C. What is the molecular weight of the gas?

STEP 1: Identify the variables given.

Identify given variables

STEP 2: Isolate the missing variable of molar mass (M).

Solving for missing variable (molar mass)Beyond Ideal Gases

To better understand the reactive nature of gases you can utilize the Kinetic-Molecular Theory and the Van der Waals equation. They help to explain concepts such as effusion rates of gasesDalton’s LawRoot Mean Square Speed, and the Simple Gas Laws

Jules Bruno

Jules felt a void in his life after his English degree from Duke, so he started tutoring in 2007 and got a B.S. in Chemistry from FIU. He’s exceptionally skilled at making concepts dead simple and helping students in covalent bonds of knowledge.