Warm Up #1 What is a gas? As the temperature of a gas increases, what happens to the speed of the gaseous molecules? Why do you think so? As the temperature.

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Presentation transcript:

Warm Up #1 What is a gas? As the temperature of a gas increases, what happens to the speed of the gaseous molecules? Why do you think so? As the temperature of a gas increases, what happens to the density of the gaseous molecules? Why do you think so?

Warm Up #2 You leave your water bottle sitting outside on a hot day, how do you think that affects the pressure inside the bottle? How can you tell? When someone sprays a strong perfume, why do you think you don’t smell its scent after a while? How do you think the pressure of air changes (if at all) as you climb a mountain? Why do you think so?

Properties of Gasses and Kinetic Energy Chapter 13.1 Properties of Gasses and Kinetic Energy

Kinetic Energy Applied Kinetic Theory – all matter in constant state of motion Kinetic = motion Kinetic Energy – energy generated due to motion/collisions Gas…no definite shape or volume Motion = constant, rapid and random Perfume smell goes away Gas particles collide (elastic) No net kinetic energy lost or gained

Pressure Pressure – created by particles colliding Vacuum – empty space with no particles and (therefore) no pressure Related to volume and temp. Barometer – used to measure gaseous pressure Units Standard Atmospheres (atm) Kilopascals (kPa) Millimeters of Mercury (mmHg) 1 atm = 760 mmHg = 101.3 kPa

Gas Pressure: Temp and Elevation Temperature – directly related to pressure As temperature INCREASES, pressure INCREASES More collisions Elevation – inversely related to pressure As elevation INCREASES, pressure DECREASES Less collisions

Kinetic Energy and Kelvin Scale oC  K = add 273 Average Kinetic Energy – avg. energy atoms of substance generate Same kinetic energy for ALL substances at given temp. Kinetic energy INCREASES with temp. More collisions Directly proportional to Kelvin scale Ex. Gas at 200 K TWICE as much energy as gas at 100 K

Quick Quiz #1 What is the difference between an inverse proportion and a direct proportion? Use relevant gas examples to explain the difference. Convert 590 mmHg into: kilopascals (kPa) and atmospheres (atm) Use the terms “average kinetic energy” and “collisions” to explain how gaseous particles respond to a decrease in temperature.