1. Gay-Lussac’s Law
The pressure of an ideal gas is directly proportional to the Kelvin temperature of the gas if the volume and moles of gas are constant.

2. GAY-LUSSAC’S LAW
As the temperature increases, the pressure increases.

3. Relationship between P and T

5. Example 1: 10. 0 L of a gas is found to exert 97. 0 kPa at 25. 0°C
Example 1: 10.0 L of a gas is found to exert 97.0 kPa at 25.0°C. What would be the required temperature (in Celsius) to change the pressure to standard pressure?
Answer: change 25.0°C to K and remember that standard pressure in kPa is Insert values into the equation (the ChemTeam will use the left-hand one in the graphic above) and get:
x = K or 38.3 oC

6. Example 2: 5. 00 L of a gas is collected at 22. 0°C and 745. 0 mmHg
Example 2: 5.00 L of a gas is collected at 22.0°C and mmHg. When the temperature is changed to standard, what is the new pressure?
Answer: convert to Kelvin and insert:
689 mm Hg

7. Combined Gas Law Equation Problems
The problem requires calculating a value for a gas property that has changed. In other words, you are asked to calculate a new pressure, temperature or volume of gas given sufficient information about the initial and other final properties.

8. Combined Gas Law Equation Problem Solving Steps
Step 1: Assign the variables P, T, and V to the values you are given and to the unknown value. Use the subscripts 1 and 2 to show initial or final conditions.
Step 2: Write out the combined gas law equation, but eliminate the variables for any constant properties. (You can assume that the properties not mentioned in the problem remain constant.)

9. Combined Gas Law Equation Problem Solving Steps
Step 3: Rearrange the equation to isolate the unknown property.
Step 4: Plug in the values for the given properties.
Step 5: Make any necessary unit conversions and cancel your units.
Step 6: Calculate your answer and report it with the correct units and significant figures.

10. Avogadro’s Law
For an ideal gas, the volume and moles of gas are directly proportional if the temperature and pressure are constant.

11. Increased Moles of Gas Leads to Increased Pressure
P  n if T and V are constant

12. Relationship between n and V

13. Engine and Pressure

14. Breathing

15. Ideal Gas Equation

16. Ideal Gas Equation Problems
In ideal gas equation questions, you are given three properties of a sample of gas and asked to calculate the fourth. Another clue is that only one gas is mentioned and there are no changing properties.

17. Ideal Gas Equation Problem Solving Steps
Step 1: Assign variables to the values given and the value that is unknown. Use P for pressure, V for volume, n for moles, T for temperature, g for mass, and M for molar mass.
Step 2: Write the appropriate form of the Ideal Gas Equation.
If the number of particles is given or desired in moles, use the most common form of the ideal gas equation.
If mass or molar mass is given or desired, use the expanded form of the ideal gas equation.

18. Ideal Gas Equation Problems
Step 3: Rearrange the equation to isolate the unknown.
Step 4: Plug in the known values, including units. Be sure to use Kelvin temperatures.
Step 5: Make any necessary unit conversions and cancel your units.
Step 6: Calculate your answer and report it to the correct significant figures and with the correct unit.

19. Combined Gas Law Equation

20. What is the volume of 1 mole of a gas at Standard Temperature and Pressure (STP)?
At STP: P = 1 atm and T = 0oC or 273 K
n = 1 mol R = L-atm
mol-K
PV = nRT
V = nRT = (1 mol) (0.082L-atm/mol-K) (273 K)
P 1 atm
= 22.4 L

21. Equation Stoichiometry

22. Dalton’s Law of Partial Pressures
The total pressure exerted by a mixture of gases is equal to the sum of the individual pressures exerted by the gases.
PT =P1 + P2 +..Pn

23. Dalton’s Law of Partial Pressures Problems
The problem involves a mixture of gases and no chemical reaction. You are asked to calculate a value for one of the variables in the equations below, and you are given (directly or indirectly) values for the other variables.

24. Dalton’s Law of Partial Pressures Problem Solving Steps
Step 1: Assign variables to the values that are given and the value that is unknown.
Step 2: From the following equations, choose the one that best fits the variables assigned in Step 1.

25. Dalton’s Law of Partial Pressures Problem Solving Steps
Step 3: Rearrange the equation to solve for your unknown.
Step 4: Plug in the values for the given properties.
Step 5: Make sure that the equation yields the correct units. Make any necessary unit conversions.
Step 6: Calculate your answer and report it with the correct units and significant figures.

26. A cylinder contains N2 and CO2
A cylinder contains N2 and CO2. The total pressure exerted by the gas mixture is 700 mm Hg. If the pressure exerted by N2 is 200 mmHg, what is the pressure of CO2?
PT =PN2 + PCO2
PCO2 =PT - PN2
= 700 mmHg – 200 mmHg = 500 mmHg

27. Graham’s Law of Diffusion
The rate at which a gas diffuse (move through open space from a region of high concentration to a region of low concentration) or effuse (move through a small opening from a region of high concentration to a region of low concentration is inversely proportional to the square root of its molar mass.
R = _1_
√MM

28. How much faster does helium move than nitrogen gas?
Solution: RHe = _ √MMN2 = √ 28 = √7 = 2.65
RN2 √MMHe √4