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PLEASE LISTEN CAREFULLY. TUTORIAL INSTRUCTIONS: Carefully go through the tutorial, step by step. You may return to any section, as necessary. - PowerPoint PPT PresentationTRANSCRIPT
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.
PLEASE LISTEN CAREFULLY
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doubling the number of particles doubles the amount of gas in the sample and halving the number of particles halves the amount of gas that is present in the sample.
LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES)
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Pressure is the force with which the gas particles bombard one unit of surface area of the container.
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At higher temperatures the average energy of the gas particles is greater and at lower temperatures the average energy of the gas particles is less.
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The volume of a gas is the volume of the container.
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IDEAL GAS LAW
PV = nRT
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When the units of pressure and volume are, respectively, atmosphere and liter, R has a value of0.082053 L
atm . mol K
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When the units of pressure and volume are, respectively, torr and milliliter, R has a value of62360.3 mL
torr . mol K
(RELATING GAS PROPERTIES)
When the units of pressure and volume are, respectively, pascal and meters cubed R has a value of8.3144 pa
m3 . mol K CLICK TO CONTINUE
(RELATING GAS PROPERTIES)
R = PV nT
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an increase in the gas pressure decreases the volume, and a decrease in gas pressure increases volume. This is called Boyle’s Law.
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an increase in the amount of gas is accompanied by a decrease in temperature, and a decrease in the amount of gas is accom-panied by an increase temperature.
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a larger gas sample will exert more pressure, a smaller gas sample will exert less pressure.
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And so, a gas sample that is composed of CO(g) at two atmospheres, Ar(g) at three atmospheres and O2(g) at one atmosphere will have a total pressure of six atmospheres.
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Dalton’s Law of Partial Pressures states that the total pressure of a mixture of gases is the sum of the partial pressures of the gasses in the mixture.
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a bigger volume of gas will have a higher temperature and a smaller volume of gas will have a lower tempera-ture. This is Charles’ Law.
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a larger gas sample will occupy a larger volume, and a smaller gas sample will occupy a smaller volume. This is Avagadro’s Law.
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an increase in temperature is accompanied by an increase in gas pressure and a decrease in the temperature is accompanied by a decreases in gas pressure. This is Gay-Lussac’s Law.
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P1V1 = P2V2
T1 T2
COMBINED GAS LAW:
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Example 1: A student prepares chlorine gas in the chemistry lab where the temperature is 20 oC, and collects it in a gas jar over water. On that day the atmospheric pressure is 0.997 atm. At 20 oC water has a vapor pressure of 17.5 torrs. What was the actual press- ure of the chlorine collected?
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The properties given are temperature (20 0C), atmospheric pressure (0.997 atm), water vapor pressure at 200 (17.5 torr). The property to be found is pressure of chlorine gas.
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Ptot = Patm = Pchlorine + Pwater vapor
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0.997 atm Pchlorine = 0.997 atm - 17.5 torr
Ptot = P1 + P2 + P3 +…
= Pchlorine + 17.5 torr
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= 0.997 atm - 17.5 torr
Ptot = Patm = Pchlorine + Pwater vapor
Ptot = P1 + P2 + P3 +…
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= Patm - Pwater vaporPchlorine
0.997 atm x 760 torrs
1 atm = 758 torrs
Pchlorine = 758 torrs – 17.5 torrs
= 740 torrs CLICK TO CONTINUE
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LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)
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Example 2: A sample of neon which occupies 40 mL at 800 torrs and 30 oC is transferred to another container in which it attains S.T.P. conditions. What is the volume of this new container?
original volume (V1) = 40 mL final volume (V2): to be determined
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LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY(ANALYSIS OF THE PROBLEM)
original pressure (P1) = 800 torrs final pressure (P2) = standard pressure = 760 torrs
original temperature (T1) = 30 0C final temperature (T2) = standard temperature = 25 0C
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P1V1 = P2V2
T1 T2
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When the final volume is determined, it will have the unit of the initial volume; the initial and final pressure units are both given in torrs; the temperature units are changed to Kelvin by adding 273:
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30 oC = (30 + 273) K = 303 K
25 oC = (25 + 273) K
= 298 K
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800 torrs x 40 mL = 760 torrs x V2
300 K 298 K
V2 = 800 torrs x 40 mL x 298 K 300 K x 760 torrs
P1V1 = P2V2 T1 T2
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V2 = P1V1T2
T1P2
= 800 torrs x 40 mL x 298 K
300 K x 760 torrs
P1V1 = P2V2 T1 T2
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V2 = 41.8 mL
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Example 3: A pure sample of CO2 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 oC the gas was at a pressure of 776 mm Hg. At what temperature was the gas originally collected?
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LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)
original volume (V1) = 2.5 L final volume (V2) = 2.5 L
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original temperature (T1) = to be determined final temperature (T2) = 27 oC
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original pressure (P1) = 1.0 atm final pressure (P2) = 776 mm Hg
P1 = P2
T1 T2
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Initial pressure:1.0 atm = 760 mm Hg
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Final temperature:27 oC = (27 + 273) K = 300 K
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EITHER
760 mm Hg = 776 mm Hg T1 300 K
T1 = 760 mm Hg x 300 K 776 mm Hg
OR
T1 = P1T2 P2
T1 = 760 mm Hg x 300 K 776 mm Hg
CLICK TO CONTINUE
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T1 = 294 K
T1 = (294 – 273) oC = 21 oC
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Example 4: A pure sample of CO2 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)
temperature of gas, T = 299 K volume of gas, V = 2.5 L
pressure of gas, P = 1.04 atm amount of gas, n: to be determined
Gas law: PV = nRT
(IDEAL GAS LAW)
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LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY(ANALYSIS OF THE PROBLEM)
R = 0.082053 L atm mol K
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EITHER
1.04 atm x 2.5 L = n x 0.082053 atm L x 299 K mol K
n = 1.04 atm x 2.5 L 0.082053 atm L mol-1 K-1 x 299 K OR
n = PV RT
n = 1.04 atm x 2.5 L
0.082053 atm L mol-1 K-1 x 299 K
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n = 0.106 mol
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mass of carbon dioxide = n x molar mass = 0.106 mol x 44.010 g/mol = 4.67 g
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volume of carbon dioxide = n x molar volume at S.T.P.= 0.106 mol CO2 x 22.414 L/mol= 2.38 L CO2 at S.T.P.
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END OF TUTORIAL
SUMMARY OF GAS LAWSGas Law Equation
Avagadro’s n/V1 = n/V2
Boyle’s P1V1 = P2V2
Charles’ V1/T1 = V2/T2
Combined P1V1/T1 = P2V2 /T2
Dalton’s Ptot = P1 + P2 + P3 +…
Gay-Lussac’s P1/T1 = P2/T2
Ideal PV = nRTCLICK TO CONTINUE
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