TUTORIAL INSTRUCTIONS: Carefully go through the tutorial, step by step. You may return to any section, as necessary. Once you are satisfied that you understand the concepts and procedures, click CLOSE to get out of the tutorial mode. You will then be taken to the post-quiz. CLICK TO CONTINUE PLEASE LISTEN CAREFULLY

Gas sample A LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES)

Amount of gas in sample B is twice as much as in sample A Gas sample B (MEASURING GASSES)

Amount of gas in sample C is half as much as in sample A Gas sample C CLICK TO CONTINUE (MEASURING GASSES)

LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES)

CLICK TO CONTINUE

Particles at temperature T LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES)

Particles at temperature higher than T (MEASURING GASSES)

Particles at temperature lower than T CLICK TO CONTINUE (MEASURING GASSES)

CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES)

IDEAL GAS LAW: PV = nRT CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING GAS PROPERTIES)

Pressure unitVolume unitValue of R atmosphereliter L atm/mol K torrmilliliter mL torr/mol K pascalmeters cubed pa m 3 /mol K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING GAS PROPERTIES)

R = PV nT CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING GAS PROPERTIES)

Boyle’s Law LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING PRESSURE, VOLUME) Twice the volume means the particles hit the container wall half as often.

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME)

Boyle’s Law (RELATING PRESSURE, VOLUME) CLICK TO CONTINUE

LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING AMOUNT, TEMPERATURE) Fewer particles mean higher temperature. CLICK TO CONTINUE T1T1 T2T2

LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING AMOUNT, PRESSURE) More particles mean more bombardments.

(RELATING AMOUNT, PRESSURE)

CLICK TO CONTINUE

Pressure of mixture = 6 atm CO(g) Ar(g) O 2 (g) ½ atmosphere gas CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (PRESSURE OF GASEOUS MIXTURE)

Partial pressure of gas 1 Partial pressure of gas 2 Partial pressure of gas 3 LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (PRESSURE OF GASEOUS MIXTURE) Dalton’s Law

Total pressure of mixture of gasses 1, 2 and 3. CLICK TO CONTINUE (PRESSURE OF GASEOUS MIXTURE) Dalton’s Law Total pressure = sum of partial pressures of gasses

Charles’ Law CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING VOLUME, TEMPERATURE) Larger volume means higher temperature. T1T1 T2T2

Avogadro’s Law CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING AMOUNT, VOLUME) More particles occupy more space.

Gay-Lussac’s Law LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING PRESSURE, TEMPERATURE) T1T1 T2T2 Higher pressure at higher temperature.

Gay-Lussac’s Law (RELATING PRESSURE, TEMPERATURE) T1T1 T2T2

Gay-Lussac’s Law (RELATING PRESSURE, TEMPERATURE) T1T1 T2T2

Gay-Lussac’s Law (RELATING PRESSURE, TEMPERATURE) T1T1 T2T2

Gay-Lussac’s Law (RELATING PRESSURE, TEMPERATURE) T1T1 T2T2

Gay-Lussac’s Law (RELATING PRESSURE, TEMPERATURE) T1T1 T2T2 CLICK TO CONTINUE

P 1 V 1 = P 2 V 2 T 1 T 2 COMBINED GAS LAW: CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING PRESSURE, VOLUME, TEMPERATURE)

CLICK TO CONTINUE Example 1: A student prepares chlorine gas in the chemistry lab where the temperature is 20 o C, and collects it in a gas jar over water. On that day the atmospheric pressure is atm. At 20 o C water has a vapor pressure of 17.5 torrs. What was the actual press- ure of the chlorine collected? LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)

Given PropertiesProperty to be found temperature = 20 0 C atmospheric pressure = atm water vapor pressure at 20 0 C = 17.5 torrs pressure of chlorine gas LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

P chlorine = atm torr P tot = P atm = P chlorine + P water vapor CLICK TO CONTINUE P tot = P 1 + P 2 + P 3 +… LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION) atm = P chlorine torr

P tot = P atm = P chlorine + P water vapor CLICK TO CONTINUE P tot = P 1 + P 2 + P 3 +… = atm torr LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION) P chlorine = P atm - P water vapor

CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (UNIT CONVERSION, EVALUATION) atm x 760 torrs 1 atm = 758 torrs P chlorine = 758 torrs – 17.5 torrs = 740 torrs

Example 2: A sample of neon which occupies 40 mL at 800 torrs and 30 o C is transferred to another container in which it attains S.T.P. conditions. What is the volume of this new container? CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)

volume (V 1 ) = 40 mL pressure (P 1 ) = 800 torrs temperature (T 1 ) = 30 o C initial properties volume (V 2 ) = ? pressure (P 2 ) = 760 torrs (standard pressure) temperature (T 2 ) = 25 o C (standard temperature) final properties CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

P 1 V 1 = P 2 V 2 T 1 T 2 CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

PropertyInitialFinal Volume Pressure Temperature mL torr ( ) K = 303 K will be mL torr ( ) K = 298 K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS, UNIT CONVERSION)

800 torrs x 40 mL = 760 torrs x V K298 K V 2 = 800 torrs x 40 mL x 298 K 300 K x 760 torrs P 1 V 1 = P 2 V 2 T 1 T 2 CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION)

V 2 = P 1 V 1 T 2 T 1 P 2 CLICK TO CONTINUE P 1 V 1 = P 2 V 2 T 1 T 2 LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION) = 800 torrs x 40 mL x 298 K 300 K x 760 torrs

V 2 = 41.8 mL CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (EVALUATION)

CLICK TO CONTINUE Example 3: A pure sample of CO 2 was collected and stored in a 2.5-liter flask on a day when the atmospheric pressure was one atmosphere. The next day when the temperature in the storage area was 27 o C the gas was at a pressure of 776 mm Hg. At what temperature was the gas originally collected? LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)

volume (V 1 ) = 2.5 L pressure (P 1 ) = 1.0 atm temperature (T 1 ) = ? o C initial propertiesfinal properties volume (V 2 ) = 2.5 L pressure (P 2 ) = 776 torrs temperature (T 2 ) = 27 o C Day 1 Day 2 CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

P 1 = P 2 T 1 T 2 CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

PropertyUnit Conversions Initial pressure1.0 atm = 760 mm Hg Final temperature27 o C = ( ) K = 300 K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (UNIT CONVERSION)

EITHER 760 mm Hg = 776 mm Hg T K T 1 = 760 mm Hg x 300 K 776 mm Hg OR T 1 = P 1 T 2 P 2 T 1 = 760 mm Hg x 300 K 776 mm Hg CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION)

T 1 = 294 K T 1 = (294 – 273) o C = 21 o C CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (EVALUATION)

Example 4: A pure sample of CO 2 was collected at 299 K and stored in a 2.5-liter flask on a day when the atmospheric pressure was 1.04 atmosphere. How much carbon dioxide was collected? CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)

gas temperature (T) = 299 K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM) gas volume (V) = 2.5 L gas pressure (P) = 1.04 atm amount of gas (n): to be determined Gas law: PV = nRT (Ideal gas law)

R = atm L mol K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

EITHER 1.04 atm x 2.5 L = n x atm L x 299 K mol K n = 1.04 atm x 2.5 L atm L mol -1 K -1 x 299 K OR n = PV RT n = 1.04 atm x 2.5 L atm L mol -1 K -1 x 299 K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION)

n = mol CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (EVALUATION)

CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING, EVALUATION) mass of CO 2 = n x molar mass = mol CO 2 x g/mol = 4.67 g

CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING, EVALUATION) = n x molar volume at S.T.P. = mol CO 2 x L/mol = 2.38 L CO 2 at S.T.P. volume of CO 2

END OF TUTORIAL SUMMARY OF GAS LAWS Gas LawEquation Avagadro’sn/V 1 = n/V 2 Boyle’sP 1 V 1 = P 2 V 2 Charles’V 1 /T 1 = V 2 /T 2 CombinedP 1 V 1 /T 1 = P 2 V 2 /T 2 Dalton’sP tot = P 1 + P 2 + P 3 +… Gay-Lussac’sP 1 /T 1 = P 2 /T 2 IdealPV = nRT CLICK TO CONTINUE

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