Chapter 10 - Review States of Matter

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Chapter 10 - ReviewStates 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?

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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?

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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?

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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?

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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?

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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 ____

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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.

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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?

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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?

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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 ____.

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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 ___.

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Chemistry Chapter 11 ReviewThermochemistry
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)

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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?

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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)

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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)

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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?

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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?

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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?

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Chapter 11 Review

• What are valid units for specific heat capacity?
• What does the symbol ?H stand for?

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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.

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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)

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Chapter 11 Review

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

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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?