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Final Jeopardy QuestionFinal Jeopardy Question
Gas LawConcepts
Gas LawProblems
500
Gas Law
DemosMisc. Gas
Laws
100
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300
400
500 500 500 500
400 400 400 400
300 300 300300
200 200 200 200
100 100 100100
STP &Temp.
Problems
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If temperature is doubled and volume is cut in half, what happens to the
pressure?
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Pressure is 4 times the original
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At constant temperature, if pressure is quadrupled, what happens to volume?
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At constant temperature, if the pressure is quadrupled, what happens to volume?
Pressure – 4x, then Volume – 1/4x
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What relationship does John’s Law demonstrate?
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Direct relationship between pressure and temperature
P1 = P2
T1 T2
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Which gas law can be represented by the following graph?
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Boyle’s Law – inverse relationship
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What does Charles’ Law state?
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At constant pressure, direct relationship between volume and
temperature
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A sample of gas has a volume of 23 mL at 39oC and 890 mm Hg. This sample is cooled down to 11oC and now has a volume of 150 mL. What is the new
pressure?
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Use the combined gas law since all variables are changing…
P1V1 = P2V2
T1 T2
890 mm Hg ( 23 mL) = P2 (150 mL)312 K 284 K
P2 = 124.22 mm HgBack
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A 50 L container is filled with a gas to a pressure of 4.7 atm at 32oC. At what
temperature IN DEGREES CELSIUS will the pressure inside the container be
3.5 atm with a volume of 50 L?
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Volume is constant, so use John’s law.
P1 = P2 4.7 atm = 3.5 atmT1 T2 305 K T2
T2 = 227.13 K – 273 = -45.87 oC
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A gas occupies a volume of 34 mL at 21.8 oC. To what temperature (in
Kelvin) must the gas be raised to have a volume of 86 mL? Assume constant
pressure.
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Pressure is constant, so use Charles’ law.
V1 = V2 34 mL = 86 mLT1 T2 294.8 K T2
T2 = 745.67 K
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A balloon has a volume of 6L at 2 atm. If the balloon was brought to a
pressure of 4 atm, what would the new volume be (assume constant temp).
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Temp is constant, so use Boyle’s law.
P1V1 = P2V2
2 atm (6L) = 4 atm (V2)
V2 = 3 LBack
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Whose law is being used in the following situation…
A sample of gas in a flexible container occupies 46.5 mL at standard pressure.
What volume will it take up if the pressure was increased to 3 atm?
Assume constant temp.
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Temp is held constant, so it is Boyle’s law.
Pressure increases while the volume decreases.
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At STP, how many liters of space will 8 g of O2 occupy?
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8 g O2 x 1 mole O2 x 22.4 L O2 = 1 32 g O2 1 mole O2 5.6 L
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What is the Kelvin value for absolute zero, and what theoretically happens at
this temperature?
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ZERO Kelvin (0K) and in theory all matter will stop moving at this temperature.
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What is 550K in oC?
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277 oC
K = 273 + oCoC = K - 273
277 oC = 550K-273
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What is 38.5 oC in Kelvin?
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311.5 K
K = 273 + 38.5oC
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What are the four values for Standard
Pressure?
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101.3 kPa = 760 torr = 760 mm Hg = 1 atm
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Explain how a straw works – and DO NOT USE THE WORD “SUCK”.
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When you inhale, your lungs expand (Volume increases), creating less pressure in the straw or your mouth. Since
the pressure in the straw is less than the pressure outside the straw, the atmospheric pressure PUSHES the
liquid into the straw so you can enjoy it!
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Explain the egg in flask demo.
AND REMEMBER SCIENCE NEVER ____!
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In the egg demo, water was heated in the flask. Since temp increased in the flask, the pressure also increased.
The flask was then taken away from the heat, and an egg was placed on top.
The flask cools down which causes the pressure inside the flask to decrease.
Since the pressure inside the flask decreased, the atmospheric pressure outside the flask was greater; therefore, it PUSHED the egg into the flask.
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A pressure apparatus that contains a sample of gas at a fixed volume is first placed into a container of hot water. It is then plunged into a container of liquid nitrogen (very cold). What happens to the pressure and why?
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This is an example of John’s law – when temp goes down, pressure
goes down.
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Explain why the Ivory soap expanded in the microwave and which gas law applies
to this situation.
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Since temp increased, so does volume. This is Charles’ law.
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What will happen to the volume of a balloon if it is placed into a bell jar
(vacuum pump) and the pump is turned on.
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The volume of the balloon will increase. This is Boyle’s law… as P decreases, V increases
and vice versa.
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At what pressure would 0.150 mole of nitrogen gas at 23.0 °C
occupy 8.90 L?
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PV = nRT (Ideal Gas Law)P = nRT V
P = .15 mol x 8.31 L*kPa x 296 K ____ mol K______
8.9L P =41.46 kPa
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How many moles of oxygen gas are contained in a 890.0 mL
container at 21.0 °C and 90.3 kPa?
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PV = nRT (Ideal Gas Law)n = PV
RT n = 90.3 kPa x .890 L
8.31 L*kPa x 294 Kmol*K
n = .032 moles O2
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What is the partial pressure of helium if the total
pressure of a rigid container is 53.1 kPa and oxygen’s
pressure in the tank is 34.3 kPa?
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P total = PHe +PO2
53.1 kPa = PHe + 34.3 kPa
PHe = 53.1 – 34.3 = 18.8 kPa
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Given the following partial pressures, solve for the total
pressure:PN2 = 22.1 kPaPO2 = 9.4 kPaPCO2 = 2.2 kPa
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P total = PN2 +PO2 +PCO2
33.7 kPa = 22.1 + 9.4 + 2.2
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2 H2O (l) 2 H2 (g) + O2 (g)
How many liters of H2 are produced if 4 L of oxygen were
produced, at STP?
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2 H2O (l) 2 H2 (g) + O2 (g)How many liters of H2 are produced if 4 L of oxygen were
produced, at STP?
4 L O2 x 1 mole O2 x 2 moles H2 x 22.4 L H2 = 8 L
1 22.4 L O2 1 mole O2 1 mole H2
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Type Question Here
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Type Answer Here
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If you are making pasta in Los Angeles and at the same time, your best friend in Colorado Springs is doing the exact same thing, whose pasta will cook first and why?
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LOS ANGELES – the boiling point of water in Los Angeles is higher than the boiling point of water in Colorado Springs. WHY?
Water boils when the vapor pressure equals the atmospheric pressure.
Because the atmospheric pressure in L.A. is higher than that in Colorado Springs, so even though the water in L.A. will boil second, it will have a higher temperature providing more heat. THUS, the pasta in L.A. will be done first.
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This Jeopardy Game was Created by: SaraFeltman, 5th Grade Teacher
Scott Elementary School1999-2000 School Year
Revised: RLipkowitz 2000