Topic: Gas Laws Aim: How do you solve Ideal Gas Laws problems?

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Presentation transcript:

Topic: Gas Laws Aim: How do you solve Ideal Gas Laws problems? Do Now: What happens to the pressure in a container when the volume is decreased?

Ideal Gases An “ideal” gas exhibits certain theoretical properties. Specifically, an ideal gas … Obeys all of the gas laws under all conditions. Does not condense into a liquid when cooled. Shows perfectly straight lines when its V and T & P and T relationships are plotted on a graph.

Ideal Gas Law Derived from Combined Gas Law # of moles of particles is directly related to pressure and volume (P1V1)/(T1n1) = R (constant) Substitute in STP values (L, kPA, K, 1 mole) Value of R?? 8.31 L kPa / K mol

Ideal Gas Law Rearrange (P1V1)/(T1n1) = R PV = nRT Only one set of conditions will be given. This calculation adjusts for the deviations of real gases from ideal conditions

Note: always use kPa, L, K, and mol in ideal gas law questions (so units cancel)

Sample problems How many moles of H2 is in a 3.1 L sample of H2 measured at 300 kPa and 20°C? How many grams of O2 are in a 315 mL container that has a pressure of 12 atm at 25°C?

Ideal Gas Law Questions How many moles of CO2(g) is in a 5.6 L sample of CO2 measured at STP? a) Calculate the volume of 4.50 mol of SO2(g) measured at STP. b) What volume would this occupy at 25°C and 150 kPa? (solve this 2 ways) How many grams of Cl2(g) can be stored in a 10.0 L container at 1000 kPa and 30°C? At 150°C and 100 kPa, 1.00 L of a compound has a mass of 2.506 g. Calculate its molar mass. 98 mL of an unknown gas weighs 0.087 g at STP. Calculate the molar mass of the gas. Can you determine the identity of this unknown gas?

98 mL of an unknown gas weighs 0. 087 g at STP 98 mL of an unknown gas weighs 0.087 g at STP. Calculate the molar mass of the gas. Can you determine the identity of this unknown gas?

(4.50 mol)(8.31 kPa•L/K•mol)(273 K) Moles of CO2 is in a 5.6 L at STP? P=101.325 kPa, V=5.6 L, T=273 K PV = nRT (101.3 kPa)(5.6 L) = n (8.31 kPa•L/K•mol)(273 K) (8.31 kPa•L/K•mol)(273 K) (101.325 kPa)(5.6 L) = n = 0.25 mol a) Volume of 4.50 mol of SO2 at STP. P= 101.3 kPa, n= 4.50 mol, T= 273 K PV=nRT (101.3 kPa)(V)=(4.5 mol)(8.31 kPa•L/K•mol)(273 K) (4.50 mol)(8.31 kPa•L/K•mol)(273 K) V = = 100.8 L (101.3 kPa)

(4.50 mol)(8.31 kPa•L/K•mol)(298 K) b) Volume at 25°C and 150 kPa (two ways)? Given: P = 150 kPa, n = 4.50 mol, T = 298 K (4.50 mol)(8.31 kPa•L/K•mol)(298 K) V = = 74.3 L (150 kPa) From a): P = 101.3 kPa, V = 100.8 L, T = 273 K Now P = 150 kPa, V = ?, T = 298 K P1V1 T1 = P2V2 T2 (101.3 kPa)(100 L) (273 K) = (150 kPa)(V2) (298 K) (101.3 kPa)(100.8 L)(298 K) (273 K)(150 kPa) = 74.3 L = (V2)

How many grams of Cl2(g) can be stored in a 10 How many grams of Cl2(g) can be stored in a 10.0 L container at 1000 kPa and 30°C? PV = nRT P= 1000 kPa, V= 10.0 L, T= 303 K (8.31 kPa•L/K•mol)(303 K) (1000 kPa)(10.0 L) = n = 3.97 mol 3.97 mol x 70.9 g/mol = 282 g At 150°C and 100 kPa, 1.00 L of a compound has a mass of 2.506 g. Calculate molar mass. PV = nRT P= 100 kPa, V= 1.00 L, T= 423 K (8.31 kPa•L/K•mol)(423 K) (100 kPa)(1.00 L) = n = 0.02845 mol g/mol = 2.506 g / 0.02845 mol = 88.1 g/mol

(neon has a molar mass of 20.18 g/mol) 98 mL of an unknown gas weighs 0.081 g at SATP. Calculate the molar mass. PV = nRT P= 100 kPa, V= 0.098 L, T= 298 K (8.31 kPa•L/K•mol)(298 K) (100 kPa)(0.098 L) = n = 0.00396 mol g/mol = 0.081 g / 0.00396 mol = 20.47 g/mol It’s probably neon (neon has a molar mass of 20.18 g/mol)