Phase Change: solid to liquid. Melting
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1
2 Phase Change: solid to liquid Melting
3 Most solids shrink in size when frozen. What substance is an exception and actually expands? water
4 Use the phase diagram below to answer the following question. What phase of matter would this substance be in at 90 C and 0.25atm? GAS A B C
5 What can cause a phase change of matter? Heat energy is either absorbed or released
6 What phase of matter is B? Liquid Pressure A B C Temperature
7 is the gas phase of a substance normally solid or liquid at room temperature Vapor
8 C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of C was decreased, the system would shift to the LEFT
9 Freezing occurs by the release of energy
10 Describe a volatile liquid in terms of its rate of evaporation. Evaporates quickly
11 is the resistance of a liquid to flow Viscosity
12 What phase of matter is A? Solid Pressure A B C Temperature
13 A is a graph of pressure versus temperature that shows which phase a substance exists in under different conditions of temperature and pressure. Phase diagram
14 What is the normal boiling point of water? 100 C
15 Melting occurs by energy being. absorbed
16 Deposition occurs when energy is (absorbed OR released). Released
17 is the temperature and pressure at which all 3 states of matter are at equilibrium Triple point
18 Phase Change: solid to gas Sublimation
19 The triple point of this substance occurs at: 5.2 atm & K
20 When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. This is known as Le Chatelier s Principle
21 C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of CO was increased, the system would shift to the LEFT
22 is the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature. Equilibrium vapor pressure
23 is the temperature at which equilibrium vapor pressure equals atmospheric pressure Boiling point
24 is a dynamic condition in which two opposing physical or chemical changes occur at equal rates in a given closed system Equilibrium
25 is the spontaneous mixing of two or more substances. Diffusion
26 When does a liquid boil? Equilibrium vapor pressure EQUALS atmospheric pressure
27 What is the most abundant liquid? Water
28 is the energy required to increase the surface area of a liquid by a given amount; results from an uneven distribution of attractive forces. Surface tension
29 List 2 examples of surface tension. Meniscus Droplets can form Objects float Capillary rise
30 List a volatile substance Rubbing alcohol Nail polish remover Gasoline hairspray
31 When energy is taken away from a substance, the particles would move Slower
32 Phase Change: liquid to solid Freezing
33 What happens to the boiling point of liquids on top of Mt. Everest? WHY? Boiling point is lower B/c atmospheric pressure is lower
34 C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 O was increased, the system would shift to the Right
35 How does a substance evaporate, if equilibrium vapor pressure is LOW? WHY? SLOWLY! B/c there are STRONG IM forces and requires MORE kinetic energy to become a vapor
36 Describe a liquid in terms of particle spacing. Particles are packed relatively closely together
37 Describe a liquid in terms of particle motion. Particles vibrate around MOVING points
38 Arrange the following in order of increasing viscosity at room temperature: tree sap, water, olive oil. Water, olive Oil, Tree Sap
39 C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 was decreased, the system would shift to the RIGHT
40 Phase Change: gas to liquid Condensation
41 Describe the general volume of a liquid and use KMT to explain. Definite VOLUME- b/c particles are close together
42 Describe the general shape of a liquid and use KMT to explain. NO Definite SHAPE- b/c particles vibrate around moving points
43 Describe a liquid-vapor system at equilibrium. The number of particles vaporizing is EQUAL to the number of particles condensing
44 Why water is considered a polar molecule? Unequal distribution of charge (oxygen is partially negative while hydrogen is partially positive)
45 Phase Change: gas to solid Deposition
46 How are boiling and evaporation alike? Both have particles changing from a liquid to a gas (vaporization)
47 Phase Change: liquid to gas Vaporization
48 What happens to the temperature of substance during a phase change? Temp. remains constant (does not change!)
49 is the transitioning from one state of matter to another. Phase change
50 Use the phase diagram below to answer the following question. What phase of matter would this substance be in at 10 C and 1.0atm? Solid A B C
51 How are boiling and evaporation different? List one difference Evaporation ONLY takes place at the surface and boiling vaporization is throughout liquid Heat is needed for boiling to occur and not for evaporation
52 Condensation occurs when energy is (absorbed OR released). RELEASED
53 What phase of matter is C? Pressure A B Gas C Temperature
54 What is the difference between the IM forces during melting and freezing? Melting = Less IM forces b/c more particle collisions Freezing = MORE IM forces b/c particles are moving slower
55 Using KMT, explain the evaporation rate of a volatile liquid. Quick evaporation rate. Has weak IM forces between particles so it requires LESS kinetic energy to become a vapor
56 Using KMT, explain the evaporation rate of a nonvolatile liquid. Slow evaporation rate Has strong IM forces between particles so it requires MORE kinetic energy to become a vapor
57 Which would you expect to be more volatile, water or rubbing alcohol? Explain. Rubbing Alcohol it evaporates quickly b/c there is WEAK IM forces between the particles
58 Explain why the solid state of water (ice) is lessdense than the liquid state. B/c of the hydrogen bondingthe arrangement of the molecules in the solid crystalline structure take up more space, yet have the same mass; making ice less dense than liquid water.
59 When energy is added to a substance, the particles would move Faster
60 Explain why the temperature remains constant during a phase change. Energy exchanges are not changes in kinetic energy so temperature remains constant. Heat energy is used to change the IM forces between the molecules
61 TRUE or FALSE: The temperature at which a substance freezes is lower than the temperature at which it melts. Why? FALSE they are the same = 0 C
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