Boyle's Law
According to Boyle's Law, the volume of a gas varies ____________ (directly/indirectly) with its pressure, assuming that temperature is held constant.
Inversely
According to Charles' Law, the volume of a gas varies ______________ (directly/indirectly) with the temperature, assuming that pressure is constant.
Directly
What three variables make up the Combined Gas Law?
Pressure, Volume, and Temperature
Why must pressure be in atm, volume be in liters, and temperature be in Kelvin when using the constant with a value of 0.0821?
Because R has units of (L*atm)/(mol*K). The units must be consistent or they will not cancel out.
Dalton's Law states that the sum of the partial pressures of all the gases that make up a mixture is equal to the __________ _________.
Total Pressure
According to Boyle's Law, the volume of a gas ___________ when the pressure increases and the temperature is held constant.
According to Charles' Law, the volume of a gas _________ when the temperature increases and the pressure is held constant.
Increases
P1 = 1.5 atm P2 = 2.5 atm
V1 = 3.0 L V2 = ?
T1 = 293 K T2 = 303 K
1.9 L
How many moles of oxygen will occupy a volume of 2.5 liters at 1.2 atm and 298 K?
0.12 mol
The partial pressures of a mixture of gasses are 22.1 torr, 169 torr, and 33.0 torr. What is the total pressure of these gasses?
223 torr
A sample of oxygen gas at constant temperature occupies a volume of 250 mL at 740 torr. What volume in mL will it occupy at 800 torr pressure?
231 mL
A sample of nitrogen occupies a volume of 0.250 L at 298 K. What volume in liters will it occupy at 368 K?
0.309 L
P1 = 720 torr P2 = ?
V1 = 0.256 L V2 = 0.250 L
T1 = 298 K T2 = 323 K
799 torr
What volume will 2.0 moles of nitrogen occupy at 0.947 atm and 293 K?
51 L
What element is used when discussing units of pressure in mm? (pressure = mm ___)
Mercury (Hg)
Ammonia gas occupies a volume of 450. mL at a pressure of 720. mm Hg. What volume in mL will it occupy at standard pressure? (760 mm Hg = 1 atm)
Hydrogen gas was cooled from 423K to 323 K. Its new volume is 0.075 liters. What was its original volume?
0.098 L
P1 = 95.0 kPa P2 = 101 kPa
V1 = 4.00 L V2 = 6.00 L
T1 = ? T2 = 471 K
295 K
At what temperature will 0.70 mol of chlorine gas exert a pressure of 900. torr at a volume of 500 mL? (1 atm = 760 torr, 1 L = 1000 mL)
10 K
A mixture of 2.00 moles of hydrogen, 3.00 moles of ammonia, 4.00 moles of carbon dioxide, and 5.00 moles of nitrogen exerts a total pressure of 800. torr. What is the partial pressure in torr of carbon dioxide?
229 torr
Fluorine gas has a volume of 317 mL. When the volume is decreased to 250. mL, its pressure is 1.50 atm. What was the original pressure in torr (760 torr = 1 atm)
899 torr
A sample of argon gas is cooled and its volume decreased from 0.380 mL to 0.250 mL. If its final temperature was 218 K, what was its original temperature in degrees Celsius?
58.25
A gas has an initial volume of 125 mL and a pressure of 125 kPa. When its volume is decreased to 100 mL and its pressure is decreased to 100 kPa, its temperature changed to 348 K. What is the initial temperature of this gas in K?
544 K
An elemental gas has a mass of 10.3 g. If the volume is 58,400 mL and the pressure is 758 mm Hg at a temperature of 2.5 oC, how many moles are present? What is the gas? (1 atm = 760 mm Hg, 1 L = 1000 mL)
n = 2.57 mol, Helium (4.0 g/mol)
A mixture of gas has 2.5 moles of Nitrogen gas (N2) and 3 moles of Chlorine gas (Cl2). The mixture of gasses have a volume of 3.5 L at a 28 oC. What is the partial pressure of Nitrogen gas?
17.6 atm