Conceptual
Pressure
Which R value would you use in this problem?
If I have 7.7 moles of gas at a pressure of 780 torrand at a temperature of 56 0 C, what is the volume of the container that the gas is in?
62.4 (L*torr/mol*K)
What equation would you use to solve this problem?
Calculate the decrease in temperature when 6.00 L at 20.0 °C is compressed to 4.00 L.
V1/T1 = V2/T2
A 40.0 L tank of ammonia has a pressure of 12.7 kPa. Calculate the volume of the ammonia if its pressure is changed to 8.4 kPa while its temperature remains constant.
Which Equation Do I Use?
P1V1 = P2V2
A gas at 260C, is ______ kelvin.
299 K
If gas is contained in a flexible container, as temperature decreases, volume __________
Decreases
What is the unit of pressure of the gas described by this equation?
(1.3 atm)(4L) = (3 mol)(0.08201)(300 K)
atm
A gas with a volume of 4.0L at a pressure of 205kPa is allowed to expand to a volume of 12.0L.
Is the new pressure going to be greater than 205 kPa, less than 205 kPa, or equal to 205 kPa?
Less than 205 kPa
If I have an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87 0 C, how many moles of gas do I have?
Which Equation Do I Use?
PV=nRT
STP (Standard Temperature and Pressure) is _____K and ______atm
273 K and 1 atm
As an airplane rises, the external air pressure is lower than the pressure inside a bag of chips. What happens to the volume of the chip bag?
The volume increases (bag expands)
If I have 4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?
204.6 K
If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume?
23.2 L
If I have 21 moles of gas held at a pressure of 78 atm and a temperature of 900 K, what is the volume of the gas?
Which Equation Do I Use?
PV=nRT
Convert 0.5 atm to torr.
380 torr
Direct
If 3.7 moles of propane are at a temperature of 28oC and are under 154.2 kPa of pressure, what volume does the sample occupy?
60 L
What is the volume of gas at 2.00 atm and 200.0 K if its original volume was 300.0 L at 0.250 atm and 400.0 K
18.75 L
A gas occupies 900.0 mL at a temperature of 27.0 °C. What is the volume at 132.0 °C?
Which Equation Do I Use?
V1/T1=V2/T2
The pressure inside a container increases as the volume of the container decreases under the same temperature and # of moles. Why?
The particles of gas will collide more frequently with the walls of the container.
As temperature increases, pressure also increases. Why is this true?
Particles are moving faster so they collide with the walls of the container more frequently AND with more force.
A sample of carbon monoxide at 57oC and under 0.67 atm of pressure takes up 85.3 L of space. What mass of carbon monoxide is present in the sample?
59 g CO
A gas is heated from 263.0 K to 298.0 K and the volume is increased from 24.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be?
0.777 atm
A gas balloon has a volume of 106.0 liters when the temperature is 45.0 °C and the pressure is 740.0 mm of mercury. What will its volume be at 20.0 °C and 780 .0 mm of mercury pressure?
Which Equation Do I Use?
(P1*V1)/T1 = (P2*V2)/T2
DAILY DOUBLE (worth 1000 points)
A 276.58-g sample of X2(g) has a volume of 30.0 L at 3.2 atm and 27°C. What is element X?
Chlorine (Cl)