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Chapter 10 Review
What is the heat in Joules required to melt 25 grams of ice? Useful information: heat of fusion of water = 334 J/g q = m·ΔHf q = (25 g)x(334 J/g) q = 8350 J
How long does it take this sample to become completely melted? About 9 minutes
Convert 705 Celsius to Kelvin 705 + 273 = 978
When a solid goes directly to a gas without becoming a liquid what is it called? Sublimation
Absolute zero is what temperature 0 Kelvin
The specific heat (c) of liquid water is 4.2 J/g 0 C. Calculate the heat necessary to change 22 g of water (l) at 5 0 C to 22 g of water (l) at 95 0 C. Q = mc T = (22)(4.2)(90) = 8316 J
Which 2 types of change require the input of thermal energy? melting, vaporizing (evaporating)
This state of matter is ionized gas and the most common form of matter in the universe Plasma
At 80 C the substance is in what state of matter? liquid
The average kinetic energy of molecules in a system is called Temperature
WHat can be said of the temperature of a substance as it undergoes a change of state It remains the same
Calculate the heat needed to change a 22 g ice cube, at 0 0 C, into 22 g of liquid at 0ºC? Heat of fusion (H f ) = 340 J/g Q = mH f = (22)(340) = 7480 J
When a substance is heated what happens to the average kinetic energy of the material? It increases
In the diagram below, at what point is the sample completely vaporized? At E
What is true about the kinetic energy in elastic collisions? It is conserved (it stays the same)
What is the triple point in a phase change diagram? The temperature point at which all three states of matter coexist
What can be said about the speed of hydrogen molecules versus nitrogen molecules if both are at the same temperature? Hydrogen molecules move faster
What is the arrangement of molecules in a solid called ? crystal lattice
The random motion of particles is called what? Brownian motion
What part of the graph shows the substance melting? BC
What does atmospheric pressure do as you go up in elevation ? decreases
The process of molecules moving from high to low concentration is called what ? diffusion
Why is glass called an amorphous solid? It does not have a crystal lattice structure
Why are gases mostly empty space? there are no attractive or repulsive forces between the gas molecules
Calculate the heat necessary to change 5 g of water (l) at 100 0 C to 5 g of vapor at 100 0 C. The heat of vaporization is 2260 J/g (5g)(2260J/g) = 22600 J
What is the triple point in the diagram? 50
The arrow represents what process? sublimation
Convert 243 K to C 273 - 243= -30 K
The specific heat (c) of solid water is 2.1 J/g 0 C. Calculate the heat necessary to change 45.5 g of water (s) at -10 0 C to 21.7 g of water (s) at 0 0 C. (45.5g)(2.1J/g)(10) = 945 J
The kinetic molecular theory describes the behavior of matter in terms of particles in motion. T or F T
Give an example of an amorphous solid Wax
When don’t gases behave like ideal gases? At extreme temperatures
Chapter 16 Section 1.
Chapter 16 Section 1 Kinetic Theory.
The Kinetic Theory of Matter
Energy and Phases. Potential Energy - stored energy (stored in bonds, height) Kinetic Energy - energy of motion, associated with heat.
3.3 Phase Changes.
Phase of Matter. Phases of Matter Gases indefinite volume and shape, low density. Liquids definite volume, indefinite shape, and high density. Solids.
Topic IV Physical Behavior of Matter
Heat & Temperature Calculations
Chapter 9- The States of Matter u Gases indefinite volume and shape, low density. u Liquids definite volume, indefinite shape, and high density. u Solids.
Chapter 10 Kinetic Theory of Matter. Objectives 10.1 Compare characteristics of a solid, liquid, and gas Relate the properties of a solid, liquid,
Kinetic Theory of Matter Why Johnny can’t sit still (Johnny is a gas particle)
Phase Changes What did one water molecule say to another water molecule about vapor? Don’t worry it’s just a phase he’ll cool down.
Chapter 10 States of Matter. Section 1: The Kinetic-Molecular Theory of Matter.
Heat and Energy J Deutsch Energy can exist in different forms, such as chemical, electrical, electromagnetic, thermal, mechanical, and nuclear.
Chapter 10 States of Matter
Chapter 13- The States of Matter u Gases- indefinite volume and shape, low density. u Liquids- definite volume, indefinite shape, and high density. u Solids-
Solids, Liquids and Gases
Kinetic Theory 16.1.
Kinetic Theory of Matter
Nature of Gases (and liquids and solids). Kinetic-Molecular Theory Assumptions Size: gases are tiny particles separated by empty space; they do not.
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