Show:
Boyle's or Charles'
Gay-Lussac or Dalton's
Ideal Gas Law or Combined Gas Law
Pressure and Temperature Conversions
Mixed Bag
100
This law states that there is an inverse relationship between pressure and volume of a gas. P1V1 = P2V2
What is Boyle's Law?
100
Total Pressure = Pa + Pb + Pc + .... is the equation for
What is Dalton's Law?
100
This gas law uses P1V1/T1 = P2V2/T2
What is the Combined Gas Law?
100
What temperature is 25oC in Kelvin?
298 K 25 + 273 = 298
100

Which law relates volume and pressure?

Boyle's law

P1V1 = P2V2

200
This law states that there is a direct relationship between a gas's volume and its temperature in Kelvin V1/T1 = V2/T2
What is Charles' Law
200
P1/T1 = P2/T2 is the equation for what law?
What is Gay-Lussac's Law?
200
This Gas Law uses PV = nRt
What is the Ideal Gas Law?
200
Express 0.830 atm in kilopascals (kPa)
0.830 atm x 101.3 kPa/1 atm = 84.1 kPa
200

As temperature increases, what will happen to volume?

Volume will increase

300
Use Boyle's Law to solve for the missing value: P1 = 350 torr V1 = 200 mL P2 = 700 torr V2 = ?
P1V1 = P2V2 (350 torr)(200 mL) = (700 torr)(V2) V2 = (350 torr)(200 mL)/(700 torr) = 100 mL
300

A gas mixture contains oxygen at 200 kPa and nitrogen at 300 kPa. What is the total pressure?

500 kPa

300
The volume of a gas is 27.5 mL at 22.0 oC and 0.974 atm. What will the volume be at 15.0 oC and 0.993 atm?
P1V1/T1 = P2V2/T2 V2 = P1V1T2/P2T1 V2 = (0.974 atm)(27.5 mL)(288 K)/(0.933 atm)(295 K) V2 = 26.3 mL
300
Express 0.83 atm in millimeters of mercury (mm Hg)
0.83 atm x 760 mm Hg/1 atm = 631 mm Hg
300

Which law is represented by the relationship between mols and Volume 

What is Avogadro's Law?

400
A flask containing a volume of 155 cm^3 of hydrogen gas was collected under pressure of 22.5 kPa. What pressure would have been required for the volume of the gas to have been 90.0 cm^3?
P1V1 = P2V2 (22.5 kPa)(155 cm^3) = (P2)(90.0 cm^3) P2 = (22.5)(155)/90 = 38.8 kPa
400
A sample of hydrogen gas at 47 oC exerts a pressure of 0.329 atm. The gas is heated to 77 oC at constant volume. What will the new pressure be?
P1/T1 = P2/T2 P2 = P1T2/T1 = (0.329 atm)(350 K)/(320 K) = 0.360 atm
400
What pressure in atmospheres (atm), is exerted by 0.325 mol of hydrogen gas in a 4.08 L container at 35 oC?
PV = nRT P = nRT/V = (0.325 mol)(0.0821)(308 K)/4.08 L P = 2.01 atm
400
Convert -30oC to Kelving
-30 + 273 = 243 K
400

What is STP? and its related values

Temperature = 0 C or 273 K 

Pressure= 1 atm, 760 mmHg, 760 torr, 101.3 KPA

500
A sample of air has a volume of 140.0 mL at 67oC. At what temperature would its volume be at 50.0 mL (constant pressure)?
V1/T1 = V2/T2 T1 = 67oC + 273 = 340K 140 mL/340 K = 50 mL/T2 T2 = (50)(340)/140 = 121 K
500

Q: A container has three gases with partial pressures:

  • Gas A = 105 kPa
  • Gas B = 153 kPa
  • Final = 600 kPa

Find missing pressure.

342 kPa 

500
Calculate the volume, in liters occupied by 2.00 mol hydrogen gas (H2) at 300.0 K and 1.25 atm.
V = nRT/P = (2.00 mol)(0.0821)(300.0 K)/1.25 atm V = 39.4 L H2
500

What is the initial temperature(in C) of Nitrous oxide if the final temperature is 386 K and the the pressure increases from 1 atm to 768 mm Hg

109 C

500

The Combined Gas Law includes which 4 Gas Laws?

Boyle's, Charles', Avogadros, and Gay-Lussac's