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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
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)
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.
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?
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
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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