Ideal+Gases

Experiments that use a large amount of gases reveal that there are four conditions to help identify the physical conditions of a gas: - temperature, //T//, pressure, //P//, volume, //V//, and the amount of gas, which is usually expressed in moles, //n//. Gas laws are obtained by holding two variables constant in order to identify the affects the remaining two variables have on each other. There are 4 specific gas laws:

1. Boyle's Law: British chemist Robert Boyle (1627-1691) was the first to investigate the relationship between the pressure of a gas and its volume. //Boyle's Law// states that the volume of a fixed quantity of gas maintained at constant temperature is inversely proportional to the pressure. **Remember that inversely proportional means that as one variable gets smaller the other variable gets bigger.**  ** Boyle's Law Equation: ** //P// denotes the pressure of the system. //V// is the volume of the gas. //k// is a constant value representative of the pressure and volume of the system.

This equation would be used when a gas starts with initial conditions of volume and pressure and then something is done to change these conditions. This equation would be used when comparing volume and pressure while keeping the number of moles and temperature constant throughout.

The relationship between pressure and volume, with a constant, temperature is shown by the first equation. The second equation illustrates the mathematical.

The equation states that, if the temperature remains constant, then the volume of a gas varies inversely as the pressure changes. - It is hard to begin inflating a balloon. A pressure of 800.0 Kpa is required to initially inflate the balloon 225.0 mL. What is the final equation for Boyle's Law. pressure when the balloon reaches it's capacity of 1.2 L?
 * Here's An Example!**

__Steps To Undergo This Problem:__ Be sure to convert all measurements to the same unit (225 mL = .225L) Plug in each pressure and volume measurement to Boyle's Equation. Equation Should Read: //800 Kpa(.225 mL) = P2 (1.2 L)// Solve for P2 //Answer = 150 Kpa.//

French scientist **Jacques Charles** (1746-1823) discovered the relationship between volume and temperature**.** //Charles's Law// states that a volume of a fixed amount of gas is //directly proportional// with temperature. Charles revealed that as gas is heated under constant pressure, it is raised one degree Celsuis and expands in volume. Basically, as one variable increases the other variable increases as well and vise versa. The pressure and moles of gas remain constant.
 * 2. Charles's Law: **



**Charles's Law Equation:**  Use this equation when initial conditions of volume and temperature are changed to final conditions. It is important to remember that all Charles's Law Equations are determined using Kelvins.

- Students conduct an experiment in which 150 mL of a gas is required at 30 degrees Celsius. What will be the volume of this gas at 15 degrees Celsius. Steps to Undergo Problem:   First, we must convert the given temperature from Celsius into Kelvin. The conversion for this is K = C + 273.15. So, 30 degrees C = 303 K & 15 degrees C = 288 K - Then plug in the volumes and temperatures given into Charles's Law equation. So, 150 mL / 303 K = X mL / 15 K - Since the temperature decreased we can assume that the volume did as well. So our answer must be less than 150 mL - Solve for x. You should have calculated an answer of about 143 mL (142.57). ** 3. Gay-Lussac's Law: French chemist** //Gay-Lussac's law// Gay-Lussac's Law Equation:
 * Here's An Example! **


 * Here's An Example!**

__Steps to Undergo this Problem:__

**4. Avogadro's Law:** //Avogadro's Law//
 * Amedeo Avogadro**

Avogardro's law states that equal volumes of gases at the same temperature and pressure contain the same number of molecules regardless of their chemical nature and physical properties. (Avogadro's number) is 6.023 X 1023 Avagardo's law makes possible determination of how much heavier a simple molecule of one gas is than that of another, as a result the relative molecular weights of gases can be ascertained by comparing the weights of equal volumes.

**Avogadro's Law Equation:** **(v=constant X n) or (n/v = constant)** **Combining all of the gases laws (**//PV=nRT)//


 * universal gas constant**


 * Here's an Example!**

__Steps to Undergo Problem__


 * Also notice that once we determine the amount of moles we must multipy that number by the molar mass of Neon because mass is determined in grams.