Gas Laws Jeopardy

Boyle's or Charles'

100

This law states that there is an inverse relationship between pressure and volume of a gas. P1V1 = P2V2

What is Boyle's Law?

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

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

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

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

Gay-Lussac or Avogadro's

100

This law has variable molar amounts

What is Avogadro's Law?

200

P1/T1 = P2/T2 is the equation for what law?

What is Gay-Lussac's Law?

300

How will you convert 1.0g of H2 to moles? 

Divide mass by molar mass of H2 (2.016g/mol)

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

500

2.0mol of gas is in a 9.0L container at constant pressure and temperature. How many moles of gas was added if the container expanded to 22.4L at constant pressure and temperature?

V1/n1 = V2/n2

(9)/(2) = (22.4)/(n2)

n2 = 4.98mol

Combined Gas Law

100

What is the constant for this law?

number of moles

200

What is the equation for this law?

This gas law uses P1V1/T1 = P2V2/T2

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

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

500

Calculate the volume, in liters from a gas that initially was held in a 5.5L container at 3.8atm and 30C that was heated to 355K with a pressure of 4.8atm.

T1 = 303K

V1P1/T1 = V2P2/T2

(5.5)(3.8)/303 = (V2)(4.8)/355

V2 = 5.1L

Pressure and Temperature Conversions

100

What temperature is 25oC in Kelvin?

298 K 25 + 273 = 298

200

Express 0.830 atm in kilopascals (kPa)

0.830 atm x 101.3 kPa/1 atm = 84.1 kPa

300

Express 0.83 atm in millimeters of mercury (mm Hg)

0.83 atm x 760 mm Hg/1 atm = 631 mm Hg

400

Convert -30oC to Kelvin

-30 + 273 = 243 K

500

Convert 2.6g of O2 to moles

2.6g x (1mol / 31.998g) = 0.081mol O2

Mixed Bag

100

What is STP? 

Standard Temperature Pressure

Temperature = 0C

Pressure = 1atm

200

What states that all particles of matter are in constant, random motion?

KMT (kinetic molecular theory)

300

Temperature is a measure of what?

Kinetic energy (KE)

400

What are 4 factors that affect gases?

Temperature, pressure, volume, moles

500

Describe what pressure is

Force of gas exerted on a given area of the container