Ideal Gas Law
What formula should be used when moles or grams are involved in a problem?
PV = nRT
5.6 L of gas is held at a pressure of 1.5 atm. If it is compressed so that the new volume is 4.8 L, what is the new pressure?
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(1.5)(5.6) = (P2)(4.8)
A gas at 14oC and a volume of 4.5 L is heated to 29oC. What is the new volume?
4.74 L
The relationship between temperature and pressure
Direct
Convert 47oC to Kelvin
320 K
What is the value for R
What is 0.0821?
A gas at a pressure of 120 kPa at a volume of 1.5 L and a temperature of 200 K is raised to a pressure of 3.5 atm at a volume of 500 mL. What is the new temperature?
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(1.18)(1.5) = (3.5)(0.5)
200 T2
A ball with 15 L of air in it at sea level (1 atm) is taken to the top of Mount Rushmore with an atm of 0.85 atm. What is the new volume?
17.65 L
When temperature increases, what happens to the speed of the particles?
increases
Convert 900 Torr to atm
1.18 atm
A 35 gram sample of N2 is placed in a 2.4 L container at 400 K.
In this problem, what value should be plugged in for n?
What is 1.25 mol?
A sample of gas at 850 mm Hg and 25oC is moved to the freezer, where temperature is 0oC. What is the pressure of the gas in the freezer?
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(1.12) = P2
298 273
A glass jar holds a gas at 699.2 mm Hg and 298 K. If the pressure is reduced to 0.61 atm, what will the temperature be?
197.59 K
Number of particles increases. DESCRIBE what happens to pressure.
More particles = more hitting the wall. Pressure increases
Convert 120 grams of NO3 to moles.
1.94 mol
4 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, The temperature is...
What is 203-205 K?
A sample of CO2 at unknown pressure is in a 500 mL balloon at 300 K. The temperature rises to 320 K, expanding the volume to 513 mL and changing the pressure to 1.5 atm. What was the initial pressure?
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(P1)0.5 = (1.5)(0.513)
300 320
A gas occupying 17 L at a pressure of 233 kPa and a temperature of 299 K is heated to 350 K, reducing the pressure to 152 kPa. What is the new volume?
30.51 Liters
Volume is decreased. DESCRIBE what happens to pressure.
Space is less.
Particles hit wall more.
Pressure increases.
The initial temperature of a sample gas in a steel container is -100.0 oC with a pressure of 0.30 atm. As the temperature increases to 103oC, calculate the final pressure of the tank.
0.65 atm
How many moles of gas are contained in a 400 mL container of a gas, held at a pressure of 10.4 atm and a temperature of 35oC?
What is 0.16 mol?
2.5 moles of a sample of H2 is held at 1.5 atm at 298 K. What is the volume of the container?
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(1.5)V = (2.5)(0.0821)(298)
2.13 L
Temperature is increased. DESCRIBE what happens to volume.
Particles speed up.
Hit wall more.
Container expands.
A gas in a 680 mL container is transferred to a 920 mL container, lowering the pressure to 3.62 atm. What was the initial pressure?
4.90 atm