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## Chapter 10 - Review States of Matter

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Title: Chapter 10 - Review States of Matter

1
Chapter 10 - Review States 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
its 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 Review Thermochemistry
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?