GASES. Identify the abundances of the naturally occurring gases in the atmosphere. Describe the historical development of the measurement of pressure.

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Presentation transcript:

GASES

Identify the abundances of the naturally occurring gases in the atmosphere. Describe the historical development of the measurement of pressure. Describe the various units used to measure pressure.

Earth’s air is composed of two types of gases: PermanentVariable Nitrogen 78.1%Water vapor 0 - 4% Oxygen 20.9%Carbon Dioxide 0.035% Argon 0.9%Methane % Neon 0.002%Ozone % Helium % Krypton % Hydrogen %

Torricelli ( ) developed the first barometer - measures air pressure Height of mercury supported by atmospheric pressure at sea level is 760 mm.

Pascal ( ) added to Torricelli’s “barometer.” Height affects the pressure of the atmosphere. Gay-Lussac ( ) observed the law of combining volumes in chemical reactions. 2 H 2 + O 2  2 H 2 O Two volumes of hydrogen combined with one volume of oxygen to form two volumes of water.

Manometer – measures gas pressure:

Vapour Pressure: P gas = P atm + h (greater than air) P gas = P atm – h (less than air)

UNITS

Dimensional Analysis Problem-solving method using relationships to change units without changing value. Relationships are made by relating two things by their equivalent "amounts" as a ratio. 1 pattyOR2 buns 2 buns 1 patty

Dimensional Analysis (Converting Units) : 1.Determine the unit ratio needed. 2. Multiply the base unit by the unit ratio. (make sure you have the new unit on top) 1.20 patty = ? buns 20 patties x 2 buns = 40 buns 1 patty 1 patty OR2 buns 2 buns 1 patty

Prefix SymbolFactor of base unitFraction of base unit gigaG billion megaM million kilo k thousand hecto h1001 hundred deca da101 ten 1 decid0.11/10 th centic0.011/100 th millim0.0011/1000 th microμ / th nanon / th

2. 3 m = ? cm 1 m or 100 cm 100 cm 1 m 3 m x 100 cm = 300 cm 1 m

3. 5 kL = ? mL 1 kL and 1 L 1000 L 1000 mL 5 kL x 1000 L x 1000 mL = mL 1 kL 1 L *need to multiply by TWO factors: kL  L  mL

1. atmosphere (atm): 1 atm = 760 mmHg = kPa 2. Pascal (Pa) – standard international (SI) units. Defined as 1 Newton of force per m 2. Use kiloPascals. 3. Millimetres of mercury (mmHg) – not common. 4. Pounds per square inch (psi) - Imperial 1 kPa is equal to psi 1 atm is equal to 14.7 psi.

P gas = 762 mm + 15 mm = 777 mmHg What is the pressure of the gas in kPa? 777 mmHg x kPa = kPa 760 mmHg

Gas pressure is due to the force of gaseous particles colliding with their container. Torricelli invented the barometer to measure atmospheric pressure. Units used: mmHg, atm, kPa, psi Using a manometer: gas pressure > air pressure P gas = P atm + h gas pressure < air pressure P gas = P atm – h.