A sample of argon gas collected at a pressure of 1.14 atm and a temperature of 1

Question

A sample of argon gas collected at a pressure of 1.14 atm and a temperature of 12.0 °C is found to occupy a volume of30.0 liters. How many moles of Ar gas are in the sample? ______ mol

A sample of krypton gas collected at a pressure of 1.13 atm and a temperature of 282 K is found to occupy a volume of619 milliliters. How many moles of Kr gas are in the sample? ______ mol

It is desired to inflate a baggie with a volume of 973 milliliters by filling it with hydrogen gas at a pressure of 0.544 atm and a temperature of 276 K. How many grams of H2 gas are needed? ______ g

Explanation / Answer

We will assume ideal gas conditions to solve all of the above problems

Ideal gas law: PV = nRT

where,

P = Pressure

V = Volume

n = number of moles

R = Gas constant = 0.0821

T = Temperature

1) A sample of argon gas collected at a pressure of 1.14 atm and a temperature of 12.0 °C is found to occupy a volume of30.0 liters

P = 1.14 atm

V = 30 L

T = 12 degree C = 285 K

PV = nRT

=> 1.14 x 30 = n x 0.0821 x 285

=> n = 1.46 moles of Ar gas

2) A sample of krypton gas collected at a pressure of 1.13 atm and a temperature of 282 K is found to occupy a volume of619 milliliters

P = 1.13 atm

V = 619 mL = 0.619 L

T = 282 K

PV = nRT

=> 1.13 x 0.619 = n x 0.0821 x 282

=> n = 0.03 moles of Kr

3) It is desired to inflate a baggie with a volume of 973 milliliters by filling it with hydrogen gas at a pressure of 0.544 atm and a temperature of 276 K

P = 0.544 atm

V = 973 mL = 0.973 L

T = 276 K

PV = nRT

=> 0.544 x 0.973 = n x 0.0821 x 276

=> n = 0.0234 moles of H2

Molar mass of H2 gas = 2 g / mol

=> Mass of H2 = 0.0234 x 2 = 0.047 g H2 is needed

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