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Gas Laws Pressurechemical, physical and conversions Boyles Law Charless Law Combined Gas Law

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Chemical Properties Produce Gases Chemists harness chemical properties to produce a desired gas through chemical reactions. Such as the reaction of zinc and hydrochloric acid.

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Physical Properties of Gases Gases are compressible and that they assume the shape and volume of any container. Gases are all infinitely soluble in one another. Each of these characteristics can be explained by the distances between the molecules (or atoms) in a gaseous sample.

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Physical Properties of Gases are affected by temperature and pressure

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Pressure Pressure is defined as force divided by the area.

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Pressure The mercury in the inverted tube is pushed upward by the force of atmospheric pressure pushing down on the surface of the mercury in the dish. The height of the mercury in the tube changes with changing atmospheric pressure. Under conditions of standard atmospheric pressure, the height of the mercury in the tube is 760 mm. (1 atm = 760 mm Hg = 760 torr = 1.01 kPa)

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Collisions cause Pressure The pressure of a gas is caused by the collision of molecules against the sides of the container.

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Low Pressure vs. High Pressure inside a System The number of collisions of gas molecules against the wall of the container determines the pressure in the container. Notice the difference in the number of collisions. Figure (a) would have a lower pressure than Figure (b).

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Robert Boyle Robert Boyle, an Irish chemist ( ), performed the first quantitative experiments on gases used a j- shaped tube to study the relationship between the pressure of the trapped gas and its volume.

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Boyles Law Boyles Law states that at constant temperature the volume of a fixed amount of gas is inversely proportional to its pressure. Boyles Law: P 1 V 1 = P 2 V 2

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Boyle Proves Changes in Pressure cause Changes in Volume As the pressure in a closed system (like a piston) decreases, the volume of the gas inside the system increases. The pressure in the system decreases exponentially. Proving an indirect relationship.

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Example: Sulfur dioxide (SO 2 ), a gas, that plays a central role in the formation of acid rain, is found in the exhaust of automobiles and power plants. Consider a 1.53 L sample of gaseous SO 2 at a pressure of 5.6 x 10 3 Pa. If the pressure is changed to 1.5 x 10 4 Pa at a constant temperature, what will be the new volume of the gas?

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Solution: P 1 V 1 = P 2 V 2 P 1 = 5.6 x 10 3 PaP 2 = 1.5 x 10 4 Pa V 1 = 1.53 LV 2 = ? Rearrange the formula to isolate V 2. P 1 V 1 = (5.6X 10 3 Pa)(1.53 L) = O.57 L P 2 (1.5 X 10 4 Pa)

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Does Boyles law really work? Since Boyles experiments (only three centuries of technological advances!) we have found that his law only holds precisely at very low pressures. We describe a gas that strictly follows Boyles law an ideal gas.

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Jacques Charles In the century following Boyle, a French physicist, Jacques Charles ( ), was the first person to fill a balloon with hydrogen gas and who made the first solo balloon flight.

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Charless Law Charless Law states that at constant pressure the volume of a fixed amount of gas is directly proportional to its absolute temperature.

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Volume vs. Temperature: Charles Law Notice the linear relationship. This relationship between temperature and volume describes a direct relationship. This means when temperature increases, so does the volume.

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The importance of 0 Kelvin At temperatures below 0 K, the extrapolated volume of gases would be negative. The fact that a gas cant have a negative volume tells us 0 K has a special significance. Absolute temperature is measured in Kelvins. At 0 K, all motion of any atom or bond ceases, therefore producing no energy. Temperatures of approximately K have been produced in laboratories, but 0 K has never been reached.

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Example: A sample of a gas at 15°C and 1 atm has a volume of 2.58 L. What volume will the gas occupy at 38°C and 1 atm? (NOTE: The pressure did not change. So you do not need to worry about it!)

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Solution: V 1 = V 2 Dont forget to convert °C to K T 1 T 2 V 1 = 2.58LV 2 =? T 1 = 15°C=288KT 2 = 38°C=311K Rearrange to solve for V 2. V 1 T 2 = (2.58L)(311K) = 2.79 L T 1 (288K)

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The Combined Gas Law The combined gas law was derived from Boyles and Charless work. A direct relationship was observed. As temperature increased, volume increased. As volume increased pressure increased. This resulted in a combined formula to calculate changes observed in a gas due to changes in either temperature, pressure or volume.

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Combined Gas Law Equation By combining the equation for Boyles Law and Charless Law. We derive the Combined Gas Law Equation where:

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Example: A sample of a gas at 15°C and 2.0 atm has a volume of 2 mL. What volume will the gas occupy at 38°C and 1 atm?

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Solution P 1 V 1 = P 2 V 2 Dont forget to convert Temperatures! T 1 T 2 P 1 = 2 atmP 2 = 1 atm V 1 =2 mLV 2 =? T 1 =15 °C=288K T 2 =38°C=311K Rearrange to solve for V 2 ! V 2 = P 1 V 1 T 2 = (2 atm)(2 mL)(311K) = 4.32 mL T 1 P 2 (288K)(1 atm)

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Summary: Boyles Law – Inverse relationship when P V and if P V Charless Law -- Direct relationship When V T and if V T

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