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Chapter 10 - Review States of Matter

Chapter 10 - Review States of Matter. Milbank High School. Chapter 10 - Review. What happens to the range of energies of the molecules in matter when the temperature is increased? What happens to the average kinetic energy of the particles in a sample of matter as the temperature is increased?.

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Chapter 10 - Review States of Matter

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  1. Chapter 10 - ReviewStates of Matter Milbank High School

  2. Chapter 10 - Review • What happens to the range of energies of the molecules in matter when the temperature is increased? • What happens to the average kinetic energy of the particles in a sample of matter as the temperature is increased?

  3. Chapter 10 - Review • Consider an iron ball and an aluminum ball. If the two balls were at the same temperature, how would their average kinetic energies compare? • Which temperature scale provides a direct measure of the average kinetic energy of a substance?

  4. Chapter 10 - Review • What instrument is normally used to measure atmospheric pressure? • What is the SI unit of pressure? • How does the atmospheric pressure at altitudes below sea level compare with atmospheric pressure at sea level?

  5. Chapter 10 - Review • What volume does 3.00 moles of gas particles occupy at STP? • What is the volume occupied by 2.20 mol of hydrogen at STP • What is the number of moles of gas in 20.0 L of oxygen at STP • What is the number of molecules of nitrogen in 11.2 L at STP?

  6. Chapter 10 - Review • What is the volume occupied by 71.0 g of chlorine gas at STP? • What is the number of grams of neon present in 78.4 L of neon at STP?

  7. Chapter 10 - Review • What happens when a gas is heated? • The average kinetic energy of the particles of a substance is proportional to the ____ of the substance. • The temperature at which the motion of particles theoretically ceases is ____

  8. Chapter 10 - Review • What is the pressure of one standard atmosphere? • Standard conditions when working with gases are defined as ____. • The pressure of a gas in a container is 152 mm Hg. This is equivalent to _____ atm.

  9. Chapter 10 - Review • Which states of matter can flow? • Which would have the greatest kinetic energy: steam at 200 oC, or water at 373 K • What happens to the evaporation rate of a liquid as the liquid is cooled?

  10. Chapter 10 - Review • If heat is added to a boiling liquid, what happens to the temperature of the liquid? • What types of forces exist between particles of a liquid?

  11. Chapter 10 - Review • The first particles to evaporate from a liquid are ____. • Which of the following will evaporate fastest: water at 20 oC, or water at 40 oC? • The direct change of a substance from a solid to a gas is called ____.

  12. Chapter 10 - Review • What is the pressure when a liquid is boiling at it’s normal boiling point? • When the vapor pressure of a liquid is equal to atmospheric pressure, the liquid ____. • Water could be made to boil at 105 oC instead of 100 oC by ___.

  13. Chemistry – Chapter 11 ReviewThermochemistry: Heat and Chemical Change Milbank High School

  14. Chapter 11 Review • How many joules are there in 148 calories? (1 cal = 4.18 J) • What is the amount of heat (in calories) required to raise the temperature of 200 g of Aluminum by 10 oC? (specific heat of Al = 0.21 cal/g x oC)

  15. Chapter 11 Review • What is the specific heat of a substance if 1560 calories is required to raise the temperature of a 312 gram sample by 15 oC?

  16. Chapter 11 Review • How much heat does it take to warm 16 g of pure water from 90.0 oC to 100.0 oC? (specific heat of water = 4.18 J / g x oC)

  17. Chapter 11 Review • When 45 g of an alloy at 52 oC is dropped into 100.0 g of water at 25 oC, the final temperature is 37 oC. What is the specific heat of the alloy? (in calories/g x oC)

  18. Chapter 11 Review • A piece of metal is heated, and then submerged into cool water. What happens to the temperature of the metal, and the temperature of the water? • How does a calorie compare to a joule?

  19. Chapter 11 Review • Two objects are sitting next to each other in direct sunlight. Object A gets hotter than object B. How does the specific heat of object A compare to object B?

  20. Chapter 11 Review • Compared to 100 g of iron, a 10 g sample of iron has _____ specific heat. • A process that absorbs heat is called a(n) _____ process. • If you were to touch the flask in which an endothermic reaction were occurring, how would it feel?

  21. Chapter 11 Review • What are valid units for specific heat capacity? • What does the symbol “H” stand for?

  22. Chapter 11 Review • Calculate the energy required to produce 7.00 mol Cl2O7 based on the following given equation: 2Cl2(g) + 7O2(g) + 130 kcal  2 Cl2O7(g) • If the heat involved in a chemical reaction has a negative sign, then heat is ____ the surroundings.

  23. Chapter 11 Review • What is the standard heat of reaction (H) for this reaction: C2H4(g) + H2(g) C2H6(g) (Hof for C2H4(g) = +52.5 kj/mol; and Hof for C2H6(g) = -84.7 kj/mol)

  24. Chapter 11 Review • The change in enthalpy is equal to _____. (give the formula)

  25. Chapter 11 Review • To determine the heat change for a reaction in an aqueous solution, _____. • What is the amount of heat needed to melt one mole of a solid called? • What is the heat of solution?

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