Presentation on theme: "Gas Laws. Charles Law V: volume, mL, cm 3, L, dm 3 T: temperature, Kelvin (T c + 273K)"— Presentation transcript:
Charles Law V: volume, mL, cm 3, L, dm 3 T: temperature, Kelvin (T c + 273K)
Example Problem #1 A. When 400mL of hydrogen at 25 o C are heated to 290 o C, what will its volume reach? B. A sample of gas at 40mL is heated to 40 o C and increases to 750mL. What is the initial temperature of the gas?
Boyles Law P: Pressure, mmHg, torr, atm, Pa, kPa V: volume, cm 3, mL, dm 3, L
Example #2 A. A 1200mL sample of oxygen at 700mmHg is expanded to 5.9L. What is the pressure at the larger volume? B. A 25mL sample of ammonia gas at 400torr is placed under a pressure of 5590torr. What is the new volume?
Gay-Lusaacs Law P: Pressure, atm, Pa, kPa, mmHg, torr T: Temperature, in Kelvin
Example #3 A. A sample of gas at 450torr at 30 o C is heated to 75 o C. What pressure will it reach? B. A sample of nitrogen at 50 o C and 2.2atm is cooled until the pressure reaches 0.8atm. What temperature did the gas reach?
Combined Gas Law All the letters are the same as before.
Example #4 A. A sample of gas at 20 o C and 800torr has a volume of 475mL. What is its volume at 75 o C and 890torr? B. A sample of gas at 35 o C and 90mmHg has a volume of 97mL. At what temperature will it reach 300mmHg with a volume of 40mL?
Ideal Gas Law P: pressure in atm V: volume in L n: moles R: (gas law constant) T: temperature in K 1 atm = 760 torr = 760 mmHg=101.4kPa
STP STP stands for standard temperature and pressure. If a problem says a gas is at STP it is actually giving you two pieces of information: P = 1atm = 760torr = 760mmHg=101.4kPa T = 273K
Example #5 A. What volume will 50g of chlorine occupy at 30 o C and 850torr? B. What pressure will 27g of carbon dioxide exert at 45 o C in a 1200mL container? C. What mass of oxygen will occupy 30mL at STP? D. What temperature will 3g of hydrogen exerts 40kPa of pressure in a 90mL container?
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Daltons Law P T = P 1 + P 2 + P 3 … P T : total pressure P 1, P 2, P 3 : partial pressures of each gas present.
Example #6 A. The total pressure in a flask is 5atm. If the flask contains 3 gases and the partial pressure of oxygen is 0.85atm, and nitrogen is 1.3atm, what is the partial pressure of the third gas in the flask?