Multiple Choice
Identify the
choice that best completes the statement or answers the question.
Important formulas and constants
Q = mDHvap
Q= mDHfus
Q = mCDT
For Water
DHfus = 6.01 kJ/mol or 334
J/g
DHvap = 40.7 kJ/mol or 2260
J/g
c = 4.18 J/goC
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1.
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Most solids ____.
a. | are able to flow | c. | are amorphous | b. | have a disorderly structure | d. | are dense and difficult to
compress |
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2.
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Which of the following examples correctly explains what happens when a bottle of
warm water is placed in a refrigerator.
a. | The air molecules in the refrigerator will transfer their cold to the water molecules
and make the water molecules move faster. | c. | The water molecules will transfer
their kinetic energy to the air molecules in the refrigerator, which causes the air molecules to move
slower and the water molecules to move faster. | b. | The water molecules will transfer their kinetic
energy to the air molecules in the refrigerator, which causes the air molecules to move faster and
the water molecules to move slower. | d. | The air molecules in the refrigerator absorb the energy from the water and turn it
into potential energy. |
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3.
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The random molecular motion of a substance is greatest when the substance is
a. | a gas. | c. | frozen. | b. | condensed. | d. | a liquid. |
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4.
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The direct change of a substance from a solid to a gas is
called...
a. | sublimation | c. | evaporation | b. | condensation | d. | boiling |
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5.
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A chunk of ice whose temperature is -20 0C
is added to an insulated cup filled with water at 0 0C. What happens in the
cup?
a. | some of the water freezes, so the chunk of ice gets
larger | c. | the ice melts until it reaches the temperature of the
water | b. | the water cools until it reaches the temperature of the
ice. |
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6.
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Particles in a gas are best described as ____.
a. | hard spheres influenced by repulsive forces from other spheres | b. | small, hard spheres
with insignificant volumes | c. | slow-moving, kinetic, hard
spheres | d. | spheres that are in fixed positions when trapped in a
container |
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7.
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A student observed that when
sodium hydroxide was dissolved in water, the temperature of the water increased. The student should
conclude that the dissolving of sodium hydroxide...
a. | produces a salt
solution | c. | produces an acid
solution | b. | is exothermic | d. | is endothermic |
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8.
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If you were to touch the flask in which an endothermic
reaction were occurring, _________.
a. | the flask would probably feel cooler than before the reaction
started | c. | the flask would probably feel warmer than before the reaction
started | b. | the flask would feel the same as before the reaction
started | d. | none of the above |
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9.
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The normal boiling point of chloroform, which has a higher vapor pressure than
water at 100  C, is ____. a. | unable to be measured | b. | lower than the normal boiling point of
water | c. | higher than the normal boiling point of water | d. | the same as the
normal boiling point of water |
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10.
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In terms of kinetic energy, how does the pressure inside a
car tire change as the air temperature outside the tire changes.
a. | an increase in temperature will decrease the pressure inside the
tire. | c. | an increase in temperature will increase the pressure inside the
tire | b. | a decrease in temperature will increase the pressure inside the
tire. |
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11.
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When the external pressure is 505 kPa, what is the vapor pressure of water at
its boiling point?
a. | 505 kPa | c. | 101.3 kPa | b. | 1010 kPa | d. | 0 kPa |
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12.
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How much heat must you add to
boil 101 g of water at
100oC?
a. | 3.34 ´ 104 | c. | 4.18 ´ 104 J | b. | 2.26 ´ 107
J | d. | 2.28 ´ 105 J |
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13.
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When 45 g of an alloy, at 25  C, are dropped into 100.0 g
of water, the alloy absorbs 956 J of heat. If the final temperature of the alloy is 37  C,
what is its specific heat? a. | 9.88  | c. | 0.423  | b. | 1.77  | d. | 48.8  |
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14.
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The graph below represents the
uniform cooling (freezing) of a substance, starting with the substance as a gas above its boiling
point.
 During which interval is the substance completely in the liquid
phase?
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15.
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During a phase change, the temperature of a substance ____.
a. | may increase or decrease | c. | decreases | b. | remains
constant | d. | increases |
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16.
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Which of the following statements is NOT true, according to the kinetic
theory?
a. | The particles of a gas collide with each other and with other
objects. | b. | Only particles of matter in the gaseous state are in constant
motion. | c. | There is no attraction between particles of a gas. | d. | All of the
statements are true. |
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17.
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Consider an iron cube and an aluminum cube. If the two cubes were at the same
temperature, how would the average kinetic energy of the particles in iron compare with the average
kinetic energy of the particles in aluminum?
a. | No determination can be made based on the information given. | b. | The average kinetic
energy of the aluminum particles would be greater. | c. | The average kinetic energy of the iron
particles would be greater. | d. | There would be no difference in the average
kinetic energies. |
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18.
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The graph below represents the
uniform cooling (freezing) of a substance, starting with the substance as a gas above its boiling
point.
 Choose the
correct formula to find the amount of heat change from D to E.
a. | Q = m(-DHfus) | d. | Q = m(-DHvap) | b. | Q = mDHvap | e. | Q = mCDT | c. | Q = mDHfus |
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19.
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A bucket of ice at 0oC absorbs just enough energy
to melt completely. It then loses just enough heat to freeze completely. The amount of
heat absorbed by the melting solid __________ the amount of heat lost by the solidifying
liquid.
a. | is less than | c. | is greater
than | b. | is the same as |
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20.
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A piece of metal is heated, then submerged in cool water. Which statement below
describes what happens?
a. | The temperature of the water will increase. | b. | The temperature of
the water will decrease. | c. | The temperature of the water will increase and
the temperature of the metal will decrease. | d. | The temperature of the metal will
increase. |
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21.
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The average kinetic energy of the particles of a substance ____.
a. | increases as the temperature of the substance is lowered | b. | is not affected by
the temperature of the substance | c. | is equal to the total energy absorbed by the
substance | d. | is directly proportional to the temperature of the
substance |
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22.
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Which states of matter can flow?
a. | gases, liquids, and solids | c. | gases only | b. | gases and liquids
only | d. | liquids
only |
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23.
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 According to the
above figure, what is happening as a substance goes from point A to point B? a. | A gas is getting colder | c. | A solid is getting
warmer | b. | Ice is melting | d. | A gas is condensing |
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24.
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What happens to the rate of evaporation of a liquid as the liquid is
cooled?
a. | It decreases. | c. | The change cannot be determined. | b. | It does not
change. | d. | It
increases. |
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25.
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Why is boiling a cooling
process?
a. | The particles with more potential energy leave the liquid first,
leaving the remaining particles with less potential energy | c. | The particles
with more kinetic energy leave the liquid first, leaving the remaining particles with less kinetic
energy | b. | The particles with less potential energy leave the liquid first,
leaving the remaining particles with more potential energy | d. | The particles with less
kinetic energy leave the liquid first, leaving the remaining particles with more kinetic
energy |
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26.
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How much heat needs to be
absorbed by 100.0 g of water at 5.0oC to raise its temperature to 75.00C?
a. | 2.93 x 104 J | c. | 175 J | b. | 1.57 x 105 J | d. | 4.18
J |
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27.
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Particles of a gas will move
a. | Slowly and predictably. | c. | In random motions, constantly
colliding with each other. | b. | In controlled, spiral
motions. | d. | Parallel to the
surface of a liquid. |
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28.
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What must happen for liquid water to freeze?
a. | The water must absorb kinetic energy from the surroundings. | c. | The water molecules
must begin to move faster | b. | The water molecules must begin to move in
random patterns. | d. | The water
must release energy to the surroundings. |
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29.
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The potential energy diagram of
a chemical reaction is shown below.
 Which letter represents the total amount of energy
released in this exothermic reaction?
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30.
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 In the above phase
diagram for carbon dioxide, carbon dioxide is a liquid at 250 C and a very high pressure.
Carbon dioxide solidifies when the temperature decreases and the pressure remains constant.
What would happen to a sample of Carbon Dioxide at a constant pressure of 0.9 atm if it were
heated from -100oC to 25oC?a. | It would melt | d. | It would sublime | b. | It would freeze | e. | It would condense | c. | It would
boil |
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31.
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When a substance condenses or freezes energy is
_______________ and when a substance evaporates or melts energy is __________________.
a. | absorbed, released | b. | released,
absorbed |
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32.
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A process that absorbs heat is a(n) ____.
a. | endothermic process | c. | ectothermic process | b. | polythermic process | d. | exothermic
process |
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33.
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Temperature on the _________ scale is directly proportional
to the average kinetic energy of the particles of a substance.
a. | Kelvin | c. | Celsius | b. | Pressure | d. | Fahrenheit |
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34.
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What happens to the average kinetic energy of the particles
in a sample of matter if the temperature of the sample is increased?
a. | it does not change | c. | it
decreases | b. | it increases |
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35.
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How much heat in kJ is absorbed
when 50.0 g of ice at 0oC
melts?
a. | 0 J | c. | 16.7 kJ | b. | 226 kJ | d. | 20.9 kJ |
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36.
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A piece of candy has 5 Calories (or 5000 calories). If it could be burned,
leaving nothing but carbon dioxide and water, how much heat would it give off?
a. | Not enough information is given. | c. | 5 kilocalories | b. | 5000
joules | d. | 500
calories |
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37.
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Water could be made to boil at 95 oC instead of
100 oC by _______.
a. | decreasing the air pressure above the water | c. | increasing the air pressure on the water | b. | decreasing the vapor pressure of the water | d. | applying a great deal of
heat |
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38.
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Heat changes can occur when ____________.
a. | a substance vaporizes | d. | a substance
solidifies | b. | a substance
melts | e. | all of the above | c. | a substance
dissolves |
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39.
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The following equation shows the reaction that occurs when
nitroglycerine explodes.
4
C3H5O9N3 à 12CO2 + 6N2 + O2 +
10H2O + 1725 kJ
This reaction is ____________.
a. | endothermic | c. | exothermic | b. | a combination
reaction | d. | a combustion reaction |
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40.
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The graph below represents the
uniform cooling (freezing) of a substance, starting with the substance as a gas above its boiling
point.
 Choose the
correct formula to find the amount of heat change from E to F.
a. | Q = mDHfus | d. | Q = m(-DHfus) | b. | Q = mCDT | e. | Q = mDHvap | c. | Q = m(-DHvap) |
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41.
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The temperature at which the motion of particles
theoretically ceases is ______?
a. | 0 K | c. | –273
K | b. | 0°C | d. | 273°C |
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42.
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The first particles to vaporize from a liquid that is
boiling are _______.
a. | those with the highest kinetic energy | c. | those farthest from the surface of the liquid | b. | those with the lowest kinetic energy |
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43.
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In a dynamic equilibrium between the liquid state and the gas state, what is
true about the rate of evaporation?
a. | The rate of evaporation cannot be determined. | b. | It is equal to the
rate of condensation. | c. | It is greater than the rate of
condensation. | d. | It is less than the rate of condensation. |
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44.
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Standard conditions when working with gases are defined as ____.
a. | 0 C and 101.3 kPa | c. | 0 C and 1
kPa | b. | 0 K and 101.3 kPa | d. | 0 K and 1 kPa |
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45.
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Which of the following usually makes a substance dissolve faster in a
solvent?
a. | agitating the solution | b. | increasing the particle size of the
solute | c. | lowering the temperature | d. | decreasing the number of
particles |
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46.
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What is the maximum amount of KCl that can dissolve in 200 g of water? (The
solubility of KCl is 34 g/100 g H 2O at 20  C.) a. | 17 g | c. | 68 g | b. | 34 g | d. | 6800 g |
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47.
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Which of the following pairs of factors affects the solubility of a particular
substance?
a. | temperature and the nature of solute and solvent | b. | temperature and
degree of mixing | c. | particle size and degree of mixing | d. | particle size and
temperature |
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48.
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Which of the following substances is less soluble in hot water than in cold
water?
a. | CO | c. | NaNO | b. | NaCl | d. | KBr |
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49.
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The solubility of a gas in a liquid is ____.
a. | proportional to the square root of the pressure of the gas above the
liquid | b. | directly proportional to the pressure of the gas above the liquid | c. | inversely
proportional to the pressure of the gas above the liquid | d. | unrelated to the
pressure of the gas above the liquid |
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50.
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In a concentrated solution there is ____.
a. | no solvent | c. | a small amount of solute | b. | a large amount of
solute | d. | no
solute |
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51.
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What is the molarity of a solution that contains 6 moles of solute in 2 liters
of solution?
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52.
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In which of the following is the solution concentration expressed in terms of
molarity?
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53.
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What is the molarity of a solution containing 7.0 moles of solute in 569 mL of
solution?
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54.
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What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide
is dissolved?
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55.
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What is the molarity of a solution containing 56 grams of solute in 959 mL of
solution? (molar mass of solute = 26 g/mol)
a. | 1.5M | c. | 2.1M | b. | 2.2M | d. | 0.0022M |
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56.
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What mass of sucrose, C  H  O  , is needed to make 500.0 mL of a
0.200 M solution? a. | 34.2 g | c. | 17.1 g | b. | 100 g | d. | 68.4 g |
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57.
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What mass of Na  SO  is
needed to make 2.5 L of 2.0 M solution? (Na = 23 g; S = 32 g; O = 16 g) a. | 178 g | c. | 356 g | b. | 284 g | d. | 710 g |
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58.
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How many mL of a 2.0M NaBr solution are needed to make 200.0 mL of
0.50M NaBr?
a. | 25 mL | c. | 100 mL | b. | 50 mL | d. | 150 mL |
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59.
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The volume of 6.00M HCl needed to make 319 mL of 6.80M HCl is
____.
a. | 0.128 mL | c. | 281 mL | b. | 7.8 mL | d. | 362 mL |
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60.
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If 2.0 mL of 6.0M HCl is used to make a 500.0-mL aqueous solution, what
is the molarity of the dilute solution?
a. | 0.024M | c. | 0.30M | b. | 0.24M | d. | 0.83M |
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61.
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To 225 mL of a 0.80M solution of KI, a student adds enough water to make
1.0 L of a more dilute KI solution. What is the molarity of the new solution?
a. | 180M | c. | 0.35M | b. | 2.8M | d. | 0.18M |
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62.
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If the percent by volume is 2.0% and the volume of solution is 250 mL, what is
the volume of solute in solution?
a. | 0.5 mL | c. | 5.0 mL | b. | 1.25 mL | d. | 12.5 mL |
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63.
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In which of the following is concentration expressed in percent by
volume?
a. | 10% (v/v) | c. | 10% (m/m) | b. | 10% (m/v) | d. | 10% |
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64.
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The volume of alcohol present in 620 mL of a 40.0% (v/v) solution of alcohol is
____.
a. | 372 mL | c. | 248 mL | b. | 40.0 mL | d. | 580 mL |
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65.
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The volume of 400 mL of chlorine gas at 400 mm Hg is decreased to 200 mL at
constant temperature. What is the new gas pressure?
a. | 400 mm Hg | c. | 800 mm Hg | b. | 300 mm Hg | d. | 650 mm Hg |
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66.
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 Which of the substances in the table can
act as either the solute or the solvent when mixed with 100 grams of water at 20 °C? a. | NH3 | c. | MgCl2
| b. | C6H5COOH
| d. | CH3 CH2OH |
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67.
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If the solubility of NaCl at 25 ºC is 36.2 g/100 g H2O, what mass of NaCl can be dissolved in 50.0 g of H2O?
a. | 18.1 g | c. | 72.4 g | b. | 36.2 g | d. | 86.2 g |
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68.
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The Dead Sea is the saltiest sea in the world. It contains 332 grams of salt
per 1000 grams of water. What is the concentration in parts per million (ppm)?
a. | 0.332 ppm | c. | 33,200 ppm | b. | 332 ppm | d. | 332,000 ppm |
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69.
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Which of these is an example of an exothermic chemical process?
a. | evaporation of water | c. | photosynthesis of glucose | b. | melting
ice | d. | combustion of
gasoline |
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70.
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A cylindrical coffee can is welded shut at
12.0oC at sea level (1 atm). Its height is 20 cm and its radius is 15 cm. If the
bursting strength of its "tin" plate is 3.75 atm, to what temperature may it be heated
before bursting?
a. | 796 oC | c. | 482
oC | b. | 45.0
oC | d. | 273oC |
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71.
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How much energy is released when 752 g of water at
its freezing point freezes?
a. | 4.18 kJ | c. | 251 kJ | b. | 3.14 kJ | d. | 752 kJ |
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72.
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 Based on the above graph, which of the
following substances show an inverse relationship between temperature and solubility?
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73.
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 Based on the above solubility graph,
how many grams of Sodium Chloride will dissolve in 1.0 L of water at 60 oC?
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74.
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 At what temperature will 1600 g of
potassium nitrate dissolve in 1.0 L of water?
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75.
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A 25.0 g sample of water at 100oC has an energy change of -1670
J. What is the new temperature of the water?
a. | 116oC | c. | 104.18oC | b. | 84.0oC | d. | 58.5oC |
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Multiple Response
Identify one
or more choices that best complete the statement or answer the question.
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76.
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Choose which example/s below are endothermic. Choose
all the apply.
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Short Answer
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77.
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It takes 770 joules of energy to raise the temperature of 50.0 g of mercury by
110  C. What is the specific heat of mercury?
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78.
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How much heat is required to raise the temperature of 5.5 
10  g of aluminum by 10  C? (specific
heat of aluminum = 0.21  )
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79.
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A 55.0-g piece of copper wire is heated, and the temperature of the wire changes
from 19.0  C to 86.0  C. The amount
of heat absorbed is 343 cal. What is the specific heat of copper?
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80.
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What is a pressure of 0.520 atm equal to in mm of Hg?
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True/False
Indicate whether the
statement is true or false.
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81.
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The melting point and the freezing point of a substance
occur at the same temperature.
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Matching
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Match each item with the correct statement below. a. | melting point | d. | evaporation | b. | boiling point | e. | vaporization | c. | sublimation | f. | normal boiling point |
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82.
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the temperature at which a solid changes into a liquid
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83.
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the change of a solid directly to a vapor
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84.
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the conversion of a liquid to a gas below the boiling point
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85.
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vaporization at the surface of a liquid that is not boiling
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86.
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the temperature at which the vapor pressure of a liquid is equal to 1
atmosphere
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87.
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the temperature at which the vapor pressure of a liquid is equal to the
external pressure
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