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Chapter_14_Gas_Laws_and_SToich

Chapter_14_Gas_Laws_and_SToich - Chapter 14 Gases A Kinetic...

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Chapter 14
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Gases A. Kinetic Theory Gas Particles do not attract or repel each other Gas particles are much smaller than distances between them
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Kinetic Theory Gas particles are in constant random motion No kinetic energy is lost when gas particles collide All gases have the same average kinetic energy at a given temperature
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B.Boyle's Law = The volume of a definite quantity of dry air is inversely proportional to the pressure, provided the temperature remains constant ( Look at page 905)
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Boyle’s Law 1.Mathematically has an inverse proportion a. V1 = P2 V2 P1 V 1 P 1 = V 2 P 2 V1 = original volume V2 = new volume P1 = original pressure P2 = new pressure
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2.Remember to solve for the unknown variable with the letters first.
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Boyle’s Law Problem 1. A 200. ml sample of H2 is collected when the pressure is 800 mm Hg. What is the volume that the H2 will occupy at 760 mm Hg?
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Boyle’s Law Problem 2 Some oxygen occupies 250. ml when the pressure is 720 mm of Hg. How many liters will the oxygen occupy when the pressure is 750 mm Hg?
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C. Charles' Law The volume of a definite quantity of dry gas varies directly with the Kelvin temperature provided the pressure remains constant.
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Charles Law Mathematically Direct Proportion a. V1 = T1 V2 T2 b. V1T2 = V2T1
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Problem example . A 22.8 cm3 volume of argon gas is collected at 48 degrees Celsius. What volume would this sample of gas occupy at standard temperature?
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