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Combined Gas Laws
Ideal Gas Laws
Random Gas Laws
Trivia Pt 1
Trivia Pt 2
100
If I start with 30 mL at 20 Celsius and heat it to 45 Celsius, what would be the new volume. (Pressure is constant)
32.6mL
100
If I have 6 moles of gas at 3.3 atm and 13 L, what would the T be?
87.1 K
100
What are the STP values for pressure (all 4 of them)
1 atm = 101.3 kPa = 760 mmHg = 760 torr
100

SING the missing parts: Equal volume of gases at the same __________ and___________, Have the ___________________________

Temp ....Pressure....Same number of molecules

100

4 identical balloons are each filled with a different gas  N2, H2, Ar, CH4.  The balloons have the same volume, pressure, and temperature. 

a. Which balloon has the greatest average kinetic energy?

b.  Which balloon has a gas with the greatest density?

c.  Which balloon has greatest average velocity?

a. All equal

b. Argon, Heavier molar mass, larger density

c.  H2  lightest

200
If I start with 0.9 atm at 10 Celsius and cool it to 3 Celsius, what would be the new pressure. (Volume is constant)
0.88 atm
200
If I have 3.7 moles of gas at 5 L and 210 K, what would the Pressure be?
12.8 atm
200
A mixture of gases with a pressure of 600.0 mmHg contains 70 percent nitrogen and 30 percent oxygen by volume What is the partial pressure of oxygen in this mixture?
180 mmHg
200

Gases will deviate from ideal gas behavior  at ______ pressure and _______ temperature.

High P  and Low T

200

A rigid 8.20 L flask contains a mixture of 2.5 mols of H2, 0.500 mols O2, and sufficient Argon so partial pressure of Ar in the flask is 2.00 atm.  The temperature is 127 C.  Calculate the total pressure in the flask.

14.0 atm

300
If I start with 14 mL at 20 Celsius and 1.2 atm, and heat it to 41 Celsius while increasing the pressure to 2.2 atm, what would be the new volume.
8.18 mL
300
If I have 22 L of gas at 3.3 atm and 280 K, how many moles do I have?
3.16 moles
300
If the total pressure of a system is 2.5 atm and the system contains the following: O at 1.4 atm, N at 0.8 atm, and F at an unknown atm, what is the partial pressure of F?
0.3 atm
300

2 H2O2(aq) -->  2  H2O(l)   +  O2(g)

The mass of an aq soln of H2O2 is 6.951g.  The O2 is collected over water at 23.4C and has a volume of 182.4mL.  The atmospheric pressure is 762.6 torr and the vapor pressure of water at 23.4C is 21.6 torr.  Calculate the number of moles of O2 produced in the reaction.

t

7.304 x 10 -3 mol

300

A rigid 8.20 L flask contains a mixture of 2.5 mols of H2, 0.500 mols O2, and sufficient Argon so partial pressure of Ar in the flask is 2.00 atm.  The temperature is 127 C.  Calculate the mole fraction of H2 in the flask

0.714

400
If I start with 17 mL at 50 Celsius and 4.2 atm, and heat it to 91 Celsius with a new volume of 3 mL, what would be the new pressure.
26.82 atm
400
If I have 0.7 moles of gas at 1.3 atm and 43 L, what would the T be?
973 K
400
How many liters are in 50 grams of Cl2 at STP?
15.8 L
400

2 H2O2(aq) -->  2  H2O(l)   +  O2(g)

The mass of an aq soln of H2O2 is 6.951g.  The O2 is collected over water at 23.4C and has a volume of 182.4mL.  The atmospheric pressure is 762.6 torr and the vapor pressure of water at 23.4C is 21.6 torr. Calculate the mass in grams of H2O2 that decomposed.

0.497 g H2O2

400

A rigid 8.20 L flask contains a mixture of 2.5 mols of H2, 0.500 mols O2, and sufficient Argon so partial pressure of Ar in the flask is 2.00 atm.  The temperature is 127 C.  Calculate the density of the mixture of the flask in g/L.

5.00 g/L

500
If I start with 44 mL at 10 Celsius and 0.2 atm, and heat it to 41 Celsius while increasing the pressure to 3.2 atm, what would be the new volume.
3.05 mL
500

What are standard conditions?

273 K  0C  and 1atm

500
Of the 3 laws, which 2 have a direct relationship (one goes up, so does the other) and which has an indirect relationship (one increases while the other decreases)?
Charles and Gay-Lussac = direct
Boyles = indirect
500

Octane, C8H18 has a denisty of 0.703g/ml at 20C.  A 255mL sample of octane reacts completely with Oxygen.  2 C8H18  +  25O2  -->  16CO2  +  18H2O

Calculate the total number of moles of gaseous products formed.

26.7 mols of product total

500

2 H2O2(aq) -->  2  H2O(l)   +  O2(g)

The mass of an aq soln of H2O2 is 6.951g.  The O2 is collected over water at 23.4C and has a volume of 182.4mL.  The atmospheric pressure is 762.6 torr and the vapor pressure of water at 23.4C is 21.6 torr. Calculate the partial pressure in torr of O2.

741.00 torr