Bell Work 1.Convert 15.3 atm to kPa 2.Convert 96.3 L of a gas at STP to moles. 3.What is the...
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Transcript of Bell Work 1.Convert 15.3 atm to kPa 2.Convert 96.3 L of a gas at STP to moles. 3.What is the...
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Bell Work1. Convert 15.3 atm to kPa2. Convert 96.3 L of a gas at STP to moles.3. What is the temperature and pressure at STP?4. A scientist is trying to determine the pressure of a
system that is made up of 4 gases. One gas has a pressure of 20 kPa. Another gas has a pressure of 5 kPa. The remaining two gases have a pressure of 2.5 kPa. What is the total pressure?
5. A system originally has a pressure of 25.2 kPa, a volume of 15.1 L and a temperature of 45.5 ˚C. What is the new volume if the pressure is decreased to 20.0 kPa and the temperature is increased to 60 ˚C?
6. How many moles are in a system that has a pressure of 2.5 atm, a volume of 33.3 L and a temperature of 75.2 ˚C?
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Homework Answers
1. 4.692. 1501 m/s3. 17.75 g/mol4. 0.485; slower5. 128 g/mol; HI6. 64 g/mol; SO2
7. 1920 m/s
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Reality Check1) In comparing the rates of diffusion of CO2
with that of Kr, which gas will diffuse faster? 2) To two decimal places, what will vA/vB (treat
this as x) be equal to if CO2 is considered to be A and Kr is considered to be B.
3) What is the molar mass of a gas if it diffuses at a rate of 647 m/s while chlorine (Cl2) gas diffuses at 840 m/s at the same temperature?
After you are finished, continue working on the lab.
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Unit 9 ReviewGases
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The Game Board
1 2 3 4 56 7 8 9 10
11 12 13 14 1516 17 18 19 2021 22 23 24 2526 27 28 29 3031 32 33 34 35
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1Calculate the approximate volume of a
2.50 mol sample of gas at -8.0°C and a pressure of 3.50 atm.
15.5 L
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2In the reaction N2 (g) + 3H2 --> 2NH3
(g), the volume ratio of H2 to N2 is___________
3 to 1
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3A pressure of 165 kPa is equal to
_____ atm.
1.63
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4What does the constant bombardment
of gas molecules against the inside of a container cause?
Pressure
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5What happens to the volume of a gas
during compression?
The Volume Decreases
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6A sample of a gas has a pressure of
2.25 atm, a volume of 650 mL and a temperature of 36°C. What would the volume of the gas be if the pressure is increased to 3.20 atm and the temperature is decreased to 31°C?
449.6 mL
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7What temperature is needed to
pressurize a 27.3 L container with 6.34 moles of air to 564.8 kPa?
292.5 K
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8When pressure, volume, and
temperature are known, the ideal gas law can be used to calculate ______________.
Molar amount (moles)
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9According to the
diagram to the right, what PV/nRT value do ideal gases have all the time?
1.0
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10What is the SI unit of pressure?
Pascal
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11If a gas with an odor is released in a
room, it quickly can be detected across the room because it ______________.
Diffuses
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12A pressure of 355000 Pa is equal to
_____ psi.
51.5
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13The principle that under similar
pressures and temperatures, equal volumes of gases contain the same number of molecules is attributed to ________________.
Avogadro
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14Nitrogen reacts with hydrogen to make
ammonia [N2 (g) + 3H2 (g) --> 2NH3 (g)]. If one needs to produce 4 L of ammonia, how many liters of nitrogen are needed?
2 L
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15A sample of a gas occupies a volume
of 1.1 L at 33°C. What temperature is needed to increase the volume of the gas to 1.9 L, if the pressure remains constant?
528.5 K or 255°C
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16A 10.5 L sample of a gas has a mass
of 95.9 g at 7.6 atm and 35°C. What is the molar mass of the gas? (Hint: divide the given mass by n).
30.4 g/mol
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17According to the
diagram to the right, at what pressure do all the gases most resemble an ideal gas?
0 atm
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18A pressure of 560 mmHg is equal to
_____ kPa.
74.7
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19Who is accredited with the idea that in
a reaction, two volumes of hydrogen gas will combine with one volume of oxygen gas to produce two volumes of water vapor?
Gay-Lussac
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20The pressure of each gas in a mixture
is called the ____________________ pressure.
Partial
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21A sample of a gas has a pressure of
567 mmHg at 23°C. What would the gas pressure be at 41°C, if the volume remains constant?
601 mmHg
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22To two decimal places, what will vA/vB
be equal to if N2 is considered to be gas A and NO is considered to be gas B. (A diffusion problem)
1.03
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23Standard temperature and pressure for
a gas is ____________________
0°C and 1 atm.
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24The total pressure of a system of four
gases is 35 atm. The first gas has a pressure of 5 atm. The second gas has a pressure of 8 atm. The remaining two pressures are the same. What is the partial pressure of the other two gases?
11
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25Charles’s law is the direct relationship
between ____________________ and volume.
Temperature
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26What is the molar mass of a gas if it
diffuses at a rate of 258 m/s while Iodine gas diffuses at 125 m/s at the same temperature?
29.7 g
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272H2O(l) + electricity 2H2(g) + O2(g)
What mass of H2O is needed to create 15.64 L of O2, if the temperature is 25°C and the pressure is 1.2 atm?
27.6 g
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28The average kinetic energy of random
motion is proportional to the temperature in what unit?
Kelvin
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29A sample of oxygen occupies 350 mL
when the pressure is 5 atm. At constant temperature, what volume does the gas occupy when pressure falls to 3 atm?
583 mL
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30Who developed the concept that the
total pressure of a mixture of gases is the sum of their partial pressures?
Dalton
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31What is the theory that explains that the
behavior of physical systems depends on the combined actions of the molecules constituting the system?
Kinetic Molecular Theory
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32A mixture of gases with a pressure of 800.0
mm Hg contains 60% nitrogen and 40% oxygen by volume. What is the partial pressure of oxygen in this mixture?
320 mm Hg
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33Line D represents water.
If the atmospheric pressure in a flask is lowered to 70 kPa, water would boil at what temperature?
92 C
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34T1 = 76 C P1 = 4 atm V1 = 560 mL
T2 = 92 C P2 = 2 atm V2 = ?
1171 mL
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35The rate of diffusion of a gas depends on the
____________ of the gas.
Molar Mass