A series of free High School Chemistry Video Lessons.

In this lesson, we will learn and apply- Boyle's Law
- Charles' Law
- Gay-Lussac's Law
- Combined Gas Law
- Ideal Gas Law

Example:

At 1.70 atm, a sample of gas takes up 4.25L. If the pressure in the gas is increased to 2.40 atm, what will the new volume be?

Example:

A sample of Ne gas occupies 0.220L at 0.86 atm. What will be its volume at 29.4kPa?

Example:

A balloon takes up 625L at 0°C. If it is heated to 80°C, what will its new volume be?

Example:

A gas at 40.0°C occupies a volume of 2.32L. If the temperature is raised to 75.0°C, what will the new volume be if the pressure is constant?

Example:

If the pressure in a car tire is 1.88 atm at 25°C, what will be the pressure if the temperature warms to 37°C?

Examples:

1. The pressure in a sealed can of gas is 235kPA when it sits at room temperature (20°). If the can is warmed to 48°C, what will the new pressure inside the can be?

2. A car tire has a pressure of 2.38 atm at 15.2°C. If the pressure inside reached 4.08 atm, the tire will explode. How hot would the tire have to get for this to happen? Report the temperature in degrees Celsius.

Example:

In the morning, a paintball pressure tank is at 306 atm. The weather heats up over the course of the day, and by 3 PM, the outside temperature is roasting at 38.5°C, and the pressure inside the tank is 324 atm. What was the temperature (in degree Celsius) in the morning?

The combined law for gases.

Example:

A gas at 110kPa at 30.0°C fills a flexible container with an initial volume of 2.00L. If the temperature is raised to 80,0°C and the pressure increases to 440Kpa, what is the new volume?

Example:

A 40.0L balloon is filled with air at sea level (1.00 atm, 25.0°C). It is tied to a riavk and thrown in a cold body of water, and it sinks to the point where the temperature is 4.0°C and the pressure is 11.0 atm. What will its new volume be?

pressure × volume = moles × ideal gas constant × temperature;

PV = nRT.

The Ideal Gas Law is ideal because it ignores interactions between the gas particles in order to simplify the equation. There is also a Real Gas Law which is much more complicated and produces a result which, under most circumstances, is almost identical to that predicted by the Ideal Gas Law.

Example:

What is the pressure in atm of a 0.108 mol sample of the gas at a temperature of 20.0°C if its volume is 0.505L?

Examples:

1) 2.3 moles of Helium gas are at a pressure of 1.70 atm, and the temperature is 41°C. What is the volume of the gas?

2) At a certain temperature, 3.24 moles of CO

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