Gas Laws Flashcards
the force exerted per unit area
pressure
common instrument for
measuring atmospheric
pressure
barometer
1 psi = ________ Pa
6894.76
1 atm = ________ Pa
101,325
1 kPa = ___ mmHg
760
1 torr = _ mmHg
1
formula for Boyle’s Law
P1V1 = P2V2
formula for Charles’
Law
V1/T1=V2/T2
formula for Gay-Lussac’s
Law
P1/T1=P2/T2
formula for Avogadro’s
Law
V1/n1=V2/n2
A gas occupies 4.31 liters at a pressure of 0.755 atm. Determine the volume if the pressure is
increased to 1.25 atm.
2.60 L
Calculate the decrease in temperature (in Celsius)
when 2.00 L at 21.0 °C is compressed to 1.00 L.
147.08 °C
If a gas in a closed container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original temperature was 25.0 °C, what would the final temperature of the gas be in degrees Celsius?
44.88 °C
A flexible container at an initial volume of 5.120 L contains 8.500 mol of gas. More gas is then added to the container until it reaches a final volume of 18.10 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.
21.55 mol
A gas occupies 12.3 liters at a pressure of 40.0 mmHg. What is the volume when the pressure is increased to 60.0 mmHg?
8.20 L
If 0.00810 mol neon gas at a particular temperature and pressure occupies a volume of 214 mL, what
volume would 0.00684 mol neon gas occupy under the same conditions?
180.71 mL
If a gas is cooled from 323.0 K to 273.15 K and the volume is kept constant, what final pressure would result if the original pressure was 750.0 mmHg?
634.25 mmHg
A gas occupies 900.0 mL at a temperature of 27.0 °C. What is the volume at 132.0 °C?
1214.84 mL
