3.4 Ideal Gas Law
Presentation
•
Science
•
11th - 12th Grade
•
Hard
Ashley Saenz
Used 2+ times
FREE Resource
21 Slides • 9 Questions
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8
Multiple Choice
Gases have...
A definite shape and volume
A definite shape but no definite volume
No definite shape but a definite volume
No definite shape or volume
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11
Multiple Choice
760 mmHg is equal to
1 torr
760 atm
760 torr
101 Pa
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Multiple Choice
What does STP (standard temperature and pressure) stand for?
0.0 degree Celcius and 1 atm
1.0 mmHg and 273 degree Kelvin
1.0 degree Celcius and 0 atm
1.0 atm 273 degree Celcius
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14
Multiple Choice
IF we are using Boyles' law and our Pressure goes UP, what must our volume do?
Go UP
Go DOWN
Stay the same
Wrong law.
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Multiple Choice
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Multiple Choice
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Multiple Choice
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28
Multiple Choice
A gas mixture at 0°C and 1.0 atm contains 0.010 mol of H2 , 0.015 mol of O2 , and 0.025 mol of N2 . Assuming ideal behavior, what is the partial pressure of hydrogen gas (H2 ) in the mixture?
about 0.010 atm, bc there is 0.010 mol H2
about 0.050 atm, bc there is 0.050 mol of gases at 0C and 1.0 atm.
About 0.20 atm, because H2
comprises 20% of the total number of moles of gas.
About 0.40 atm, because the mole ratio of H2 :O2 :N2 is 0.4:0.6:1.
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Multiple Choice
An equimolar mixture of N2 (g) and Ar(g) is kept inside a rigid container at a constant temperature of 300 K. The initial partial pressure of Ar in the mixture is 0.75 atm. An additional amount of Ar was added to the container, enough to double the number of moles of Ar gas in the mixture. Assuming ideal behavior, what is the final pressure of the gas mixture after the addition of the Ar gas?
0.75atm, because increasing the partial pressure of Ar decreases the partial pressure of N2
1.13atm, because 33% of the moles of gas are N2 .
1.50atm, because the number of moles of N2 did not change.
2.25atm, because doubling the number of moles of Ar doubles its partial pressure
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