Gases - General Properties of Gases
Gases: Examine the properties of real and ideal gases. Perform calculations using the Ideal Gas Law, Dalton's Law, Graham's Law, and Van der Waals Equation. Learn to prepare gases in the lab.
General Properties of Gases
All pure substances display similar behavior in the gas phase. At 0° C and 1 atmosphere of pressure, one mole of every gas occupies about 22.4 liters of volume. Molar volumes of solids and liquids, on the other hand, vary greatly from one substance to another. In a gas at 1 atmosphere, the molecules are approximately 10 diameters apart. Unlike liquids or solids, gases occupy their containers uniformly and completely. Because molecules in a gas are far apart, it is easier to compress a gas than it is to compress a liquid. In general, doubling the pressure of a gas reduces its volume to about half of its previous value. Doubling the mass of gas in a closed container doubles its pressure. Increasing the temperature of a gas enclosed in a container increases its pressure.
Because different gases act similarly, it is possible to write a single equation relating volume, pressure, temperature, and quantity of gas. This Ideal Gas Law and the related Boyle's Law, Law of Charles and Gay-Lussac, and Dalton's Law are central to understanding the more complex behavior of real gases.
Ideal Gas Law:
PV = nRT
Boyle's Law:
PV = k1
Law of Charles and Gay-Lussac:
V = k2T
Dalton's Law:
Ptot = Pa + Pb
where:
P is pressure, Ptot is total pressure, Pa and Pb are component pressures
Problem
2.50 g of XeF4 gas is placed into an evacuated 3.00 liter container at 80°C. What is the pressure in the container?
Solution
PV = nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature.
P=?
V = 3.00 liters
n = 2.50 g XeF4 x 1 mol/ 207.3 g XeF4 = 0.0121 mol
R = 0.0821 l·atm/(mol·K)
T = 273 + 80 = 353 K
Plugging in these values:
P = nRT/V
P = 00121 mol x 0.0821 l·atm/(mol·K) x 353 K / 3.00 liter
P = 0.117 atm
General Properties of Gases
All pure substances display similar behavior in the gas phase. At 0° C and 1 atmosphere of pressure, one mole of every gas occupies about 22.4 liters of volume. Molar volumes of solids and liquids, on the other hand, vary greatly from one substance to another. In a gas at 1 atmosphere, the molecules are approximately 10 diameters apart. Unlike liquids or solids, gases occupy their containers uniformly and completely. Because molecules in a gas are far apart, it is easier to compress a gas than it is to compress a liquid. In general, doubling the pressure of a gas reduces its volume to about half of its previous value. Doubling the mass of gas in a closed container doubles its pressure. Increasing the temperature of a gas enclosed in a container increases its pressure.
Because different gases act similarly, it is possible to write a single equation relating volume, pressure, temperature, and quantity of gas. This Ideal Gas Law and the related Boyle's Law, Law of Charles and Gay-Lussac, and Dalton's Law are central to understanding the more complex behavior of real gases.
Ideal Gas Law:
PV = nRT
Boyle's Law:
PV = k1
Law of Charles and Gay-Lussac:
V = k2T
Dalton's Law:
Ptot = Pa + Pb
where:
P is pressure, Ptot is total pressure, Pa and Pb are component pressures
Problem
2.50 g of XeF4 gas is placed into an evacuated 3.00 liter container at 80°C. What is the pressure in the container?
Solution
PV = nRT, where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature.
P=?
V = 3.00 liters
n = 2.50 g XeF4 x 1 mol/ 207.3 g XeF4 = 0.0121 mol
R = 0.0821 l·atm/(mol·K)
T = 273 + 80 = 353 K
Plugging in these values:
P = nRT/V
P = 00121 mol x 0.0821 l·atm/(mol·K) x 353 K / 3.00 liter
P = 0.117 atm
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