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Chapter 10 - Review States of Matter

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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 ... – PowerPoint PPT presentation

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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?
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