# IDEAL gas law.

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IDEAL gas law

Solve quantitative problems involving the relationships among the pressure, temperature, and volume of a gas using dimensional analysis. Include: Avogadro, Ideal Gas Law and the mole Additional KEY Terms Molar volume Molar mass

Avogadro ( ) Any sample of any gas at the same temperature and pressure will contain the same number of particles.

* Experiment conducted at constant temperature and pressure

Particles are now counted in moles (n).
Defined 22.4 L as the molar volume for any gas. Particles are now counted in moles (n). The number of moles is directly proportional to pressure, temperature, and volume.

P1 V1 = P2 R k V2 n T1 T2 L · kPa 8.314 mol · K
Experiments with n, V, P, and T give Ideal gas law: P1 V1 = P2 R k V2 n T1 T2 R = experimentally determined ideal gas constant. Value of R depends on the units used for pressure. L · atm L · kPa 0.0821 8.314 mol · K mol · K L · mmHg 62.4 mol · K

A steel container with a volume of 20
A steel container with a volume of 20.0 L is filled with nitrogen gas to a final pressure of kPa at 27.00C. How many moles of gas was used? L · kPa mol · K 8.314 = P V n R T 27°C = 300 K = 2000 (20.0) 16.0 moles n 8.314 (300)

The mass of 1 mole is the molar mass - (g/mol)
One mole of any particle has a mass equal to its total formula mass – IN GRAMS. The mass of 1 atom of Al = 27.0 µ The mass of 1 mole of Al atoms = 27.0 g The molecular mass of water (H2O) is 18.0 µ ... So...the molar mass of water is 18.0 g/mol.

Molar mass of lead (II) chloride, PbCl2 ?
1 particle of PbCl2 - 1 atom of Pb, 2 atoms of Cl 1 mole of PbCl2 - 1 mole of Pb, 2 moles of Cl PbCl2 = g/mol + 2(35.5 g/mol) = g/mol The molar mass of lead (II) chloride is g/mol.

What pressure is exerted by 640.0 g of methane (CH4) gas in a sealed 5.35L container at 27 ºC?
Molar mass of CH4 = 16.0 g/mol 640.0 g 16.0 g 1 mol = moles L · kPa mol · K 8.314 P V = n R T 27°C = 300 K (40.0) 8.314 (300) 1.9 x 104 kPa = (5.35)

= 2.75 g of O2 = P V n R T = 101.3 (2.2) 0.086 moles 8.314 (310)
A child lung capacity is 2.2 L. How many grams of oxygen gas do lungs hold at a pressure of 1.00 atm and a normal body temperature of 37.00C? L · kPa mol · K 8.314 = P V n R T 37°C = 310 K = 101.3 (2.2) 0.086 moles 8.314 (310) Molar mass of O2 = 32.0 g/mol 1 mol 32.0 g 0.086 mol = g of O2

CAN YOU / HAVE YOU? Solve quantitative problems involving the relationships among the pressure, temperature, and volume of a gas using dimensional analysis. Include: Avogadro, Ideal Gas Law and the mole Additional KEY Terms Molar volume Molar mass