1.  Reactions that require energy are called what?  Which phase changes release energy?  What is the triple point of a substance?  What are 3 units of pressure for a gas?

2. Pg. 95 foldable

3.  Number of gas particles present  Temperature  Pressure  Volume  Be sure to watch units!

4.  Definition- the volume of a gas held at a constant temperature varies INVERSLY with pressure  Decrease in volume represents an increase in pressure  Formula- P 1 V 1 =P 2 V 2  Example: The volume of a gas at 99 kPa is 300.00 mL. If the pressure is increased to 188 kPa, what will be the new volume?

5.  Definition- the volume of a gas is DIRECTLY proportional to its Kelvin temperature at constant pressure.  Volume goes increases, temperature increases  Formula- V 1 /T 1 =V 2 /T 2 or V 1 T 2 =V 2 T 1  Converting from Celsius to Kelvin- C +273  Example- A gas at 89 o C occupies a volume of.67 L. At what Celsius temperature will the volume increase to 1.12 L?

6.  Definition- the pressure of a gas is DIRECTLY proportional with temperature if volume is held constant.  Formula- P 1 /T 1 =P 2 /T 2 or P 1 T 2 = P 2 T 1  Example: A gas in a sealed container has a pressure of 125 kPa at a temperature of 30.0 o C. If the pressure in the container is increased to 201 kPa, what is the new temperature?

7.  Definition- states the relationship of temp, press, and vol, for a fixed amount of gas. All variables have the same relationship as in other gas laws.  Formula- P 1 V 1 /T 1 = P 2 V 2 /T 2  Example: A helium filled balloon at sea level has a volume of 2.1 L at 0.998 atm and 36 o C. If it is released and rises to an elevation at which the pressure is 0.900 atm and the temperature is 28 o C, what will be the new volume?

8.  Definition- describes the physical behavior of an ideal gas in terms of pressure, temperature, volume, and number of moles present.  Ideal- assumes have no intermolecular attraction  Formula – PV=nRT  R is the ideal gas constant = 0.0821 (if P is in atm)= 8.314 (if P is in kPa)  n= the number of moles  Example- If the pressure exerted by a gas at 25 o C in a volume of 0.044 L is 3.81 atm, how many moles of gas are present?

9.  Can find molar mass  n= given mass/mm  Formula  PV=mRT/mm  Can find density  d=m/v  Formula  P(mm)/RT=m/v Example: How many grams are present in a sample that has a molar mass of 70 g/mol and occupies a 2.00 L container at 117 kPa and 35.1 o C. Example: What is the density of a gas at 1.0 atm at 22 o C that has a molar mass of 44 g/mol?