Chapter 10 - Review States of Matter by F3514Gb

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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
  increased?
• What happens to the average
  kinetic energy of the particles in a
  sample of matter as the
  temperature is increased?
       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?
       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?
       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?
       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?
       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 ____
       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.
        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?
        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?
         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
  ____.
       Chapter 10 - Review
• What is the pressure when a liquid
  is boiling at it’s 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 ___.
Chemistry – Chapter 11 Review
 Thermochemistry: Heat and
      Chemical Change

       Milbank High School
       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)
       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?
       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)
       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)
       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?
       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?
        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?
       Chapter 11 Review


• What are valid units for specific
  heat capacity?
• What does the symbol “H” stand
  for?
       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.
        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)
       Chapter 11 Review


• The change in enthalpy is equal to
  _____. (give the formula)
       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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