worksheet Ideal Gas Law

1 atm = 101.3 kPa = 760 mm Hg ;

K = 273 + C ;

1 L = 1,000 mL ;

R = 0.0821 (atm.L)/(mol.K)

PV=NRT

Answers to one decimal point unless otherwise instructed

NO UNITS !!!

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What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20 C?

ANSWER to 2 Decimal points on this one ,remember no units... such as 0.99

Oxygen gas is collected at a pressure of 123 kPa in a container which has a volume of 10.0 L. What temperature must be maintained on 0.500 moles of this gas in order to maintain this pressure? Express the temperature in degrees

R= 8.314 kpa L/mol K

How many moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of 100.C? R=8.314 kpa l/mol k

2 decimal places on this one , also

After determining the number of moles, calculate the number of grams of chlorine (Cl2) contained in this container? Use 35 for the mass of Cl

What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20. C and standard pressure?

Calculate the volume which 1.00 mole of a gas occupies at STP.

What volume would 22.0g of CO2 occupy at a temperature of 25 C and a pressure of 105 kPa? (use 44 for the CO2)

A 23.6g sample of an unknown gas occupies a volume of 12.0 L at standard temperature and pressure. What is the molecular mass of this gas? Hint:find the number of moles first then use that info and the number of grams to find the molecular mass

What pressure would a sample of gas have if the volume is 10.0 L the amount of gas is 0.10 moles, and the temperature is 500. Kelvin?

Pressure in atmospheres. Use two decimal points, no units in answer. for instance: 0.26