1. CHAPTER 10 TEST REVIEW SHEET

2. 1. The kinetic-molecular theory of gases assumes that the particles of an ideal gas are separated by great distances. This implies that the gas particles are considered to have no definite_____________________. 2. If the particles in a sample of matter are attracted to each other but can move past each other easily, the matter is a _____________________. 3. According to the equation for the kinetic energy of a moving object, gases with the ________________ mass will have the lowest average velocity. 4. Which factor is the most important in determining the average kinetic energy of gas particles? 5. Sublimation involves changing from a _____________________ to a _____________________. 1. VOLUME 2. LIQUID 3. HIGHEST 4. VOLUME OF THE CONTAINER 5. SOLID TO GAS

3. 6. Liquids and solids are much denser than gases because the particles of liquids and solids have a ________. 7. An increase in pressure exerted on a liquid does not compress the liquid as much as the same increase in pressure compresses a gas because _____________________. 8. When there is a small decrease in temperature, the average kinetic energy of the particles of a liquid_____ 9. Amorphous solids behave like liquids at certain temperatures because of their ______________________. 10. What is the relationship between the melting and freezing points of a pure substance? 6. CLOSER ARRANGEMENT 7. PARTICLES ARE MORE CLOSELY PACKED IN LIQUIDS 8. DECREASES 9. RANDOM ARRANGEMENT OF PARTICLES 10. THEY ARE THE SAME TEMPERATURE

4. 11. A phase diagram relates the state of matter, pressure, and _____________________ 12. On a phase diagram, the point at which all equilibrium lines join is the _____________________ 13. According to the kinetic-molecular theory, how do particles of an ideal gas move? 14. As atmospheric pressure on the surface of a liquid decreases, its boiling point _____________________ 11. TEMPERATURE 12. TRIPLE POINT 13. ELASTICALLY COLLIDE, BUT DON’T ATTRACT EACH OTHER 14. DECREASES

5. 15. According to the phase diagram shown above, if you had a container of the substance at room temperature (approximately 25 degrees Celsius) what phase would you expect to find it in? 15. GAS OR LIQUID DEPENDING ON THE PRESSURE

6. 16. If a substance was at 10 degrees Celsius and 500 mm Hg pressure, and there was an increase to a temperature of 100 degree Celsius without changing pressure, what phase change would have happened? 16. EVAPORATION

7. 17. If remaining at a constant pressure, what type of temperature (high or low) would produce a phase with the highest molecular kinetic energy? 17. HIGH TEMPERATURE

8. 18. Mr. Grubb doesn’t like to drink warm water. The water bottle on his desk is currently sitting at 23 degrees Celsius. How many joules of energy would be needed to cool his water bottle down to 3 degrees Celsius, assuming that it contains 500 grams of water? SHOW WORK AND FINAL ANSWER ON YOUR ANSWER SHEET ONLY PLEASE. 18. Q= S x M x ∆T Q = 4.18 x 500 x (3-23) Q = -41,800 JOULES

9. 19. Mr. Grubb made a giant ice sculpture of a glorious unicorn. The body of the beast is composed of 200,000 grams of ice (water). The head and mane total 50,000 grams of ice (water). How much energy is required to melt the mythic stallion to liquid water? SHOW WORK AND FINAL ANSWER ON YOUR ANSWER SHEET ONLY PLEASE. 19.Q = m x H f Q = 250,000 x 334 = Q = 83,500,000 Joules

12. 20. Flavor Ice’s are an amazing summertime treat to beat the heat. However, they are best served icy cold. Suppose you have a 500 gram flavor ice that is still liquid and at room temperature of 25 degrees Celsius. How much energy would it take to freeze the Flavor Ice to a chilly -25 degrees? SHOW WORK AND FINAL ANSWER ON YOUR ANSWER SHEET ONLY PLEASE. 20. Q= S x M x ∆T so 4.18 x 500 x (0-25) = -52,250 AND Q = M x Hf so 500 x 334 = 167,000 AND Q= S x M x ∆T So 2.1 x 500 x (-25-0) = -26,250 AND: -52,250 + 167,000 - 26,250 = 88,500J