Matter and Energy Review Packet
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1 Name Date Matter and Energy Review Packet 1. A compound differs from a mixture in that a compound always has a (1) homogeneous composition (2) maximum of two components (3) minimum of three components (4) heterogeneous composition 2. The phase change represented by the equation: I2 (s) à I2 (g) is called (1) sublimation (2) condensation (3) melting (4) boiling 3. Which phase change is exothermic? (1) solid to liquid (2) solid to gas (3) liquid to solid (4) liquid to gas 4. As electrical energy is converted into heat energy, the total amount of energy (1) decreases (2) increases (3) remains the same 5. Which change results in a release of energy? (1) melting of H2O (s) (2) boiling of H2O (l) (3) evaporation of H2O (l) (4) condensation of H2O (g) 6. Which statement is an identifying characteristic of a mixture? (1) it consists of a single element (2) it can be separated by physical means (3) it has definite composition by weight (4) it is always homogeneous 7. Which of the following represents a homogeneous mixture? (1) CuSO4 (s) (2) Br2 (l) (3) NaCl (aq) (4) CO2 (g) 8. Which Kelvin temperature is equal to - 73 C? (1) 100 K (2) 173 K (3) 200 K (4) 346 K 9. Which change in the temperature of a 1- gram sample of water would cause the greatest increase in the average kinetic energy of its molecules? (1) 1 C to 10 C (2) 10 C to 1 C (3) 50 C to 60 C (4) 60 C to 50 C 10. The graph below represents the relationship between temperature and time as heat is added uniformly to a substance. Which portions of the graph represent times when heat is absorbed and potential energy increases while kinetic energy remains constant? (1) A and B (2) B and D (3) A and C (4) C and D
2 11. Which physical changes are endothermic? (1) melting and freezing (2) melting and evaporating (3) condensation and sublimation (4) condensation and deposition 12. Which term represents a form of energy? (1) heat (2) degree (3) kilocalorie (4) temperature 13. How many joules of heat are required to raise the temperature of 20 grams of water from 30 C to 40 C? (1) 42 J (2) 84 J (3) 420 J (4) 840 J 14. If 420 joules are added to 20 grams of water at 30 C, what will be the final temperature of the water? (1) 25 C (2) 35 C (3) 40 C (4) 50 C 15. The temperature of 50 grams of water was raised to 50 C by the addition of 4,200 joules of heat energy. What was the initial temperature of the water? (1) 10 C (2) 20 C (3) 30 C (4) 60 C 16. When a 500 gram sample of water at 19 C absorbs 8.40 kilojoules of heat, the temperature of the water will change to (1) 23 C (2) 19 C (3) 15 C (4) 4 C 17. The heat of fusion for ice is 334 J/g. Adding 334 joules of heat to one gram of ice at STP will cause the ice to (1) increase in temperature (2) decrease in temperature (3) change to water at a higher temperature (4) change to water at the same temperature 18. The heat of fusion of a substance is the energy measured during a (1) phase change (2) temperature change (3) chemical change (4) pressure change 19. What is the total number of kilojoules of heat needed to change 150 grams of ice to water at 0 C? (1) 50.1 kj (2) 2.22 kj (3) 184 kj (4) 484 kj 20. Twenty five grams of a compound at its normal boiling point is converted to a gas by the addition of 34,400 joules. What is the heat of vaporization for this compound? (1) 25 J/g (2) 1,376 J/g (3) 2,260 J/g (4) 34,400 J/g
3 Part 2 Questions 1. Explain how you would determine if a particle diagram represented an element, compound or mixture. 2. What is the difference between physical and chemical properties? Physical and chemical changes? 3. Describe the 3 phases of matter in terms of shape, volume, and particle arrangement. 4. Draw a heating curve and indicate the phase(s) present, what is happening to kinetic and potential energy, and the phase changes that occur. Also include important points such as melting point, freezing point, and boiling point. 5. When given a heat calculation question, how do you know which equation to use?
4 Answer Key Part 2 1. Element: single circles or 2 identical circles attached; every particle must look the same Monoatomic Diatomic Compound: 2 or more different colored circles attached; every particle must look the same Mixture: at least 1 particle must look different 2. Physical Property: observed without changing identity, ex color Chemical Property: changes identity, ex reactivity Physical Change: no new substance forms, ex phase changes, dissolving Chemical Change: new substance forms, ex burning, rusting 3. Solid: definite shape, definite volume, particles arranged very close together Liquid: indefinite shape, definite volume, particles arranged randomly and close together Gas: indefinite shape, indefinite volume, particles arranged randomly and far apart
5 4. boiling pt. melting pt. freezing pt. AB: solid present, KE changes, PE constant BC: solid and liquid present (melting/freezing), KE constant, PE changes CD: liquid present, KE changes, PE constant DE: liquid and gas present (boiling/condensation), KE constant, PE changes EF: gas present, KE changes PE constant 5. Look for key words - q = mc T: temperature change, 2 temperatures given q = mhf: melting, fusion, freezing, ice, 0 C q = mhv: boiling, vaporizing, condensing, steam, 100 C } Do not plug in temperatures
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