Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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A substance that does NOT conduct an electric current when it forms a solution
is a(n) ____.
a. | electrolyte | c. | liquid | b. | nonelectrolyte | d. | solid |
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2.
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A solution that contains all of the solute it can hold at a given temperature is
____.
a. | diluted | c. | supersaturated | b. | saturated | d. | unsaturated |
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3.
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When a gas is dissolved in a liquid, the gas dissolves faster if the liquid is
____.
a. | cooled | c. | heated | b. | an electrolyte | d. | under low
pressure |
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4.
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Which of the following combinations would increase the solubility of a gas in a
liquid?
a. | Decrease the pressure and decrease the temperature. | b. | Decrease the
pressure and increase the temperature. | c. | Increase the pressure and decrease the
temperature. | d. | Increase the pressure and increase the temperature. |
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5.
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Which of the following will speed up the dissolving of a solid solute in
water?
a. | Cool the solution. | c. | Grind up the solvent. | b. | Freeze the
solute. | d. | Stir the
solution. |
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6.
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When one element replaces another element in a compound, the reaction is a ____
reaction.
a. | decomposition | c. | single–displacement | b. | double–displacement | d. | synthesis |
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7.
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A substance that speeds up a chemical reaction without being permanently changed
itself is a(n) ____.
a. | catalyst | c. | inhibitor | b. | coefficient | d. | reactant |
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8.
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What type of reaction is shown in the following chemical equation:
2H2O ® 2H2 + O2?
a. | decomposition | c. | single–displacement | b. | double–displacement | d. | synthesis |
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9.
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____ change color in the presence of an acid or a base.
a. | Acids | c. | Buffers | b. | Glycerins | d. | Indicators |
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10.
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Coffee has a pH of about 5. Coffee is ____.
a. | extremely acidic | c. | somewhat acidic | b. | extremely basic | d. | somewhat basic |
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11.
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Increasing the surface area of a solid ____.
a. | causes the solid to ionize | c. | slows the rate of
solution | b. | has no effect on the rate of solution | d. | speeds the rate of
solution |
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12.
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Increasing temperature generally increases the solubility of a solute in a
solvent.
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13.
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In a solution, the substance that is being dissolved is the ____.
a. | gas | c. | solute | b. | liquid | d. | solvent |
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14.
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If two liquids are soluble in each other, they are said to be _____.
a. | soluble | c. | miscible | b. | insoluble | d. | immiscible |
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15.
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The substance in a solution that dissolves another substance is called
___.
a. | solute | c. | electrolyte | b. | solvent | d. | nonelectrolyte |
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16.
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According to the graph above, about how many grams of KBr are needed to make a
saturated soultion in 100 g of water at 30° C?
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17.
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According to the graph above, which salt is more soluble in water KCl or
KBr?
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18.
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According to the graph above, at what temperature is the solubility of KBr the
same as KNO3?
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19.
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According to the graph above, what kind of solution would you have if you
dissolved 10 g of KCl in 100 g of water at 0°C?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | polysaturated |
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20.
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According to the graph above, which of the following substance’s
solubility increases the least as temperature goes up?
a. | potassium nitrate | c. | potassium chloride | b. | potassium bromide | d. | sodium chloride |
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21.
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According to the graph, how many grams of KCl wil form a saturated solution in
100 g of water at 60°C?
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SOLUBILITY OF SUBSTANCES IN WATER AT
20°C | Solid Substances | Solubility in g/100 g of
Water | Barium sulfate
Lithium carbonate
Potassium chloride
Sodium
nitrate
Lithium bromide | 0.00025
1.3
34.0
87.6
166.0 | | |
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22.
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According to the chart above, what type of solution would you have if 1.5 g of
lithium carbonate is dissolved in 100 g of water at 20 °C?
a. | saturated | c. | unsaturated | b. | supersaturated | d. | polysaturated |
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23.
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According to the chart above, what type of solution would you have if 166.0 g of
lithium bromide is dissolved in 100 g of water at 20 °C?
a. | saturated | c. | unsaturated | b. | supersaturated | d. | polysaturated |
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24.
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A mixture with particles that will settle out if left undisturbed is a(n)
___.
a. | suspension | c. | colloid | b. | emulsion | d. | electrolyte |
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25.
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A solution in which the solvent is water is called ___.
a. | concentrated | c. | aqueous | b. | dilute | d. | amphoteric |
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26.
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A solution is made by dissolving 17.0 g of Lithium iodide in enough water to
make 500.0 mL of solution. What is the molarity of the solution?
a. | 34 M | c. | 0.25 M | b. | 0.034 M | d. | 2.54 x
10-4 |
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27.
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Calculate the molarity of a water soluiton of CaCl2 made by
dissolving 612 g of CaCl2 in 5.04 L of solution.
a. | 1.09 M | c. | 0.775 M | b. | 22.0 M | d. | 1.88 M |
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28.
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What is the molarity of an aqueous solution containing 40.0 g of glucose
(C6H12O6) in 1.5 L of solution?
a. | 27 M | c. | 0.22 M | b. | 60 M | d. | 0.15 M |
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29.
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What is the molarity of an aqueous solution containing 14.2 g of NaCl dissolved
in 2000 mL of solution?
a. | 7.1 M | c. | 0.12 M | b. | 0.24 M | d. | 3.6 M |
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30.
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____________ are the products of a neutralization reaction between a strong acid
& a strong base.
a. | water & acid | c. | water & salt | b. | base & salt | d. | acid & base |
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31.
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A ___ solution contains more hydroxide ions that it does hydrogen ions.
a. | acidic | c. | neutral | b. | basic | d. | saturated |
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32.
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Since nitric acid is a ____ acid, it ionizes completely in solution
a. | concentrated | c. | strong | b. | dilute | d. | weak |
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33.
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The negative logarithm of the hydrogen ion concentration is ___.
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34.
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The substances produced when KOH neutralizes HCl are
a. | KH + ClOH | c. | KClH + OH | b. | KCl + H2O | d. | HOH +
KCl2 |
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35.
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Which expression represents the pH of a solution?
a. | log [H+] | c. | antilog
[-pOH] | b. | - log [H+] | d. | -antilog
[pOH] |
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36.
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Which is a strong base?
a. | H2O | c. | NaOH | b. | CH4 | d. | HCH3COO |
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37.
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The formula for the products between sodium hydroxide and sulfuric acid are
___.
a. | NaSO4 + H2O | c. | NaS2 +
H2O | b. | Na2SO4 + H2O | d. | NaH + SOH |
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38.
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If 50.0 ml of a 0.500 M solution of HCl is diluted to 150.0 ml, what will the
final molarity be?
a. | 0.667 | c. | 1.50 | b. | 5.99 | d. | 0.167 |
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39.
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What would the final volume of a solution be if 5.0 mL of a 0.040 M stock
solution is diluted to 0.030 M?
a. | 6.67 | c. | 0.00244 | b. | 0.150 | d. | 416 |
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40.
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What explains the solubility of ionic substances in water?
a. | water is polar | c. | water is poly polar | b. | water is nonpolar | d. | water dissolves
everything |
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41.
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A chemist is having some difficulty getting a yellow crystalline solid compound
to dissolve in water. What strategy might she employ to increase the solubility of the
solid?
a. | heat the solution | c. | shake it | b. | grind up the solid | d. | all of these would
work |
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42.
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A student pours a sample of a clear liquid – whose identify is unknown
– into a test tube of water. The water and the liquid form two distinct layers, with the
unknown on the bottom. What is true of the system?
a. | the two solutions are miscible | c. | the density of the unknown liquid
is less dense than the water | b. | the unknown solution is non
polar | d. | the two are soluble
in each other |
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43.
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Weak acids and bases produce what type of ions in solution?
a. | many | c. | H+ ions only | b. | only a few | d. | OH- ions
only |
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44.
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8 KClO3 +
C12H22O11 ® 8 KCl
+ 12 CO2 + 11 H2O
If 3.0 moles of potassium chlorate
are used, how many moles of water would be produced?
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45.
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8 KClO3 +
C12H22O11 ® 8 KCl
+ 12 CO2 + 11 H2O
If 25.0 g of carbon dioxide
are produced, how many grams of sugar (C12H22O11) were used?
a. | 0.0473 | c. | 16.2 | b. | 21.1 | d. | 0.0617 |
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46.
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8 KClO3 +
C12H22O11 ® 8 KCl
+ 12 CO2 + 11 H2O
How many grams of sugar
(C12H22O11) were oxidized by the potassium chlorate, if 3.16 g of
water were produced?
a. | 0.183 | c. | 62.7 | b. | 0.0159 | d. | 5.46 |
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47.
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8 KClO3 +
C12H22O11 ®8 KCl +
12 CO2 + 11 H2O
How many moles of potassium chlorate
are required to produce 18.0 g of water?
a. | 89.0 | c. | 54.1 | b. | 0.726 | d. | 6.72 |
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48.
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What is a reaction in which oxygen combines with a substance and releases heat
and light known as?
a. | single replacement | c. | synthesis | b. | double replacement | d. | combustion |
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49.
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Ammonia (NH3) is used to make fertilizer. If you have 2.00 x 10
3g of N2 how many grams of ammonia can be
produced?
N2 +
3H2 à
2NH3
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50.
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Calculate the number of moles in 250.0g of potassium chlorate
(KClO3).
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51.
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Determine the molar mass of KC2H3O2.
a. | 68.12 | c. | 86.14 | b. | 98.15 | d. | 82.15 |
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52.
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Determine the number of moles in 25.50 g Ag.
a. | 0.236 | c. | 3.64 x 10-4 | b. | 2750 | d. | 4.24 |
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53.
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Given 3.25 mol of AgNO3, determine the number of formula
units.
a. | 0.0191 | c. | 1.96 x 1024 | b. | 5.40 x
10-24 | d. | 52.4 |
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54.
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Given the following combustion reaction of a hydrocarbon, balance the equation
and determine the coefficient of
H2O.
C4H6 + O2 ®
CO2 + H2O
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55.
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How many atoms of Cu are in 4.00 moles?
a. | 254 | c. | 2.41 x 1024 | b. | 0.00393 | d. | 6.64 x
10-24 |
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56.
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How many grams of CCl4 are in 4.00 moles? The formula mass of
carbon tetrachloride is 153.8 g/mol.
a. | 0.026 | c. | 2.41 x 1024 | b. | 615 | d. | 4.15 x
10-25 |
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57.
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How many grams of CH3Br could be made from 10.0 g of CH3OH
and excess PBr3?
3 CH3OH +
PBr3 à 3
CH3Br + P(OH)3
a. | 23.4 | c. | 4.27 | b. | 0.0428 | d. | 0.234 |
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58.
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How many grams of ZnCl2 are produced from 75.00 g of ZnO in the
reaction
ZnO + 2HCl ® ZnCl2 + H2O ?
a. | 44.79 | c. | 125.6 | b. | 0.0223 | d. | 0.00796 |
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59.
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How many hydrogen atoms are there in 1.0 x 102 g of glucose,
C6H12O6?
a. | 0.555 | c. | 3.34 x 1023 | b. | 4.01 x
1024 | d. | 2.49 x
10-25 |
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60.
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How many moles are in 1.2 X 1024 molecules of water?
a. | 0.503 | c. | 7.72 x 1047 | b. | 1.38 x
10-48 | d. | 1.99 |
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61.
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How many moles of CH3Br could be made from 3.0 moles of
PBr3 and excess
CH3OH?
3 CH3OH +
PBr3 à 3
CH3Br + P(OH)3
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62.
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If the pressure exerted by a gas at 25.0o C in a volume of 0.0440 L
is 3.81 atm, how many moles of gas are present? (Hint: R = 0.0821 L-atm/mol-K)
a. | 0.00685 | c. | 12.2 | b. | 0.0817 | d. | 146 |
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63.
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In the equation HCl + KOH ® KCl +
H2O, how many grams of water are produced if 3.000 moles of HCl are used?
a. | 0.166 | c. | 54.06 | b. | 6.01 | d. | 0.0185 |
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64.
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In the reaction 2Na + Cl2 ®
2NaCl, how many grams of sodium chloride can be produced from 120.0 g of sodium in the presence
of excess chlorine?
a. | 305 | c. | 0.0212 | b. | 47.2 | d. | 0.00328 |
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65.
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One in a series of reactions that inflates airbags in automobiles is the
decomposition of sodium azide
(NaN3).
2 NaN3 (s) ® 2 Na (s)
+ 3 N2 (g)
Determine
the mass of N2 produced if 1.00 x 102 g NaN3 is decomposed.
a. | 21.5 | c. | 0.00215 | b. | 464 | d. | 64.64 |
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66.
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What is the coefficient that belongs in front of carbon dioxide in the
equation?
____C3H8 + ___O2 ®
____CO2 + ___H2O
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67.
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What is the correct molar mass of Ca(OH)2 ?
a. | 74.1 | c. | 58.11 | b. | 57.09 | d. | 60.75 |
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68.
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The
following reaction is an example of which type of reaction?
AgNO3(aq) + NaCl
(aq) ® AgCl(s)
+ NaNO3(aq)a. | synthesis | c. | single replacement | b. | decomposition | d. | double
replacement |
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69.
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What is the formula mass of (NH4)3PO4?
a. | 121.1 | c. | 144.07 | b. | 149.12 | d. | 153.20 |
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70.
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The molar mass of CO2 is 44 g/mol. How many moles are present
in 110 g?
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71.
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The molar mass of H2O is 18.015 g/mol. How many moles of water
are present in 3.6 g?
a. | 0.015 | c. | 5.00 | b. | 64.85 | d. | 0.20 |
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72.
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The molar mass of NH3 is 17.0 g/mol. How many grams of NH3
are present in 3.50 moles?
a. | 59.5 | c. | 0.210 | b. | 0.0170 | d. | 4.85 |
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73.
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What type of reaction is 2Hg + O2 ®
2HgO?
a. | single replacement | c. | synthesis | b. | double replacement | d. | decomposition |
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74.
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What are the coefficients to correctly balance the formula equation
Pb(NO3)2 (aq) + KI (aq) ® PbI2 (s) + KNO3(aq)
a. | 1 2 1 2 | c. | 1 4 1 4 | b. | 2 1 2 1 | d. | 4 1 4 1 |
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75.
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What are the coefficients to correctly balance the formula equation
AlCl3(aq) + Pb(NO3)2(aq) ® PbCl2(s) +
Al(NO3)3(aq)
a. | 3 2 3 2 | c. | 1 7 4 2 | b. | 2 3 3 2 | d. | 5 1 1 2 |
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76.
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What is the balanced equation when aluminum reacts with
copper(II)sulfate?
a. | Al + CuSO4 ® Cu +
AlSO4 | c. | 4Al + 3Cu2(SO4)2 ®
6Cu + 2Al2(SO4)3 | b. | 2Al + 3CuSO4 ® 3Cu + Al2(SO4)3 | d. | 2Al +
Cu2(SO4)2 ® 2Cu +
2AlSO4 |
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77.
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What volume of oxygen is needed to completely combust 2.36 L of methane gas
(CH4)?
CH4 (g) + 2 O2
(g) ®CO2
(g) + 2 H2O (g)
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78.
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A container of gas at 550.0 mm Hg and 35.0°C is
heated to 60.0°C. What is the new pressure in mm Hg?
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79.
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A container of gas at 760.0 mm Hg and 20.0°C is
heated to 40.0°C. What is the new pressure in mm Hg?
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80.
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A gas at 740.0 mm Hg pressure at 25.0 °C is
cooled to –10.0 °C. What is the final pressure in mm
Hg?
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81.
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A gas at 925.0 mm Hg pressure at 50.00 °C is
cooled to –25.00 °C. What is the final pressure in
mm Hg?
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82.
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A sample of ammonia gas occupies a volume of 1.58 L at 22.0o C and a
pressure of 0.983 atm. What volume will the sample occupy at 1.00 atm and 0
oC?
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83.
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A sample of ammonia gas occupies a volume of 27.4 L at 14.0o C and a
pressure of 1.20 atm. What volume will the sample occupy at 3.00 atm and 0 oC?
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84.
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A sample of gas at 1.50 atm and 4.0 L is compressed to 2.5 L at a constant
temperature. What is the new pressure?
a. | 6.67 | c. | 0.417 | b. | 0.938 | d. | 2.4 |
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85.
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A sample of gas at 2.50 atm and 6.50 L is compressed to 1.50L at a constant
temperature. What is the new pressure?
a. | 10.8 | c. | 3.9 | b. | 0.092 | d. | 0.577 |
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86.
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A sample of gas at 255 K occupies a volume of 1.55 L. If the temperature is
raised to 298 K what will be the new volume?
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87.
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A sample of gas at 313 K occupies a volume of 2.32 L. If the temperature is
raised to 348 K what will be the new volume?
a. | 2.58 | c. | 04.29 | b. | 2.09 | d. | 0.388 |
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88.
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A sample of SO2 gas has a volume of 1.16 L at a temperature of
23o C. At what temperature will the gas have a volume of 1.25 L?
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89.
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A sample of SO2 gas has a volume of 9.50 L at a temperature of 320K.
At what temperature will the gas have a volume of 2.55 L?
a. | 27.2 | c. | 1192 | b. | 0.865 | d. | 85.9 |
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90.
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A student collects 285 mL of O2 gas at a temperature of
15.0°C and a pressure of 99.9 kPa. The next day the
sample occupies 292 mL at a temperature of 11.0o C, What is the new pressure of the
gas?
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91.
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A student collects 355 mL of O2 gas at a temperature of 27°C and a pressure of 127 kPa. The next day the sample occupies 257 mL
at a temperature of 17o C, What is the new pressure of the gas?
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92.
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Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a
pressure of 0.900 atm.
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93.
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Determine the Kelvin temperature required for 0.0470 mole of gas to fill a
balloon to 1.20 L under 0.988 atm pressure.
a. | 30.7 | c. | 0.0033 | b. | 307 | d. | 0.033 |
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94.
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Determine the temperature of 2.49 moles of gas contained in a 2.00L vessel at a
pressure of 1.41 atm.
a. | 0.073 | c. | 1.37 | b. | 0.73 | d. | 13.7 |
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95.
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What is the final pressure in atm, if 10.0 L of gas at 25.0°C and 1.00 atm pressure is compressed to 2.00 L at 323°C?
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96.
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What is the final pressure in atm, if 5.25 L of gas at 75.0°C and 1.33 atm pressure is compressed to 2.75 L at 155 °C?
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97.
|
What is the pressure in atmospheres of a 0.108 mole sample of helium gas at a
temperature of 20.0°C if its volume is 0.505 L?
a. | 0.351 | c. | 5.14 | b. | 2.85 | d. | 0.194 |
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98.
|
What pressure will be needed to change the volume of 22.4 L of helium at 25.0
kPa to a volume of 85.0L?
a. | 0.013 | c. | 0.0105 | b. | 76.2 | d. | 94.9 |
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99.
|
What pressure will be needed to reduce the volume of 77.4 L of helium at 98.0
kPa to a volume of 60.0L?
a. | 0.013 | c. | 47.4 | b. | 126 | d. | 0.021 |
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100.
|
You have 200.0 cm3 of nitrogen (IV) oxide at a temperature of 303.0 K
and a pressure of 101.0 kPa. What volume will the NO2 occupy at 255.0 kPa and 371.0
K?
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101.
|
You have 422.0 cm3 of nitrogen (IV) oxide at a temperature of 295.15
K and a pressure of 101.325 kPa. What volume will the NO2 occupy at 155.00 kPa and 317.15
K?
a. | 0.0069 | c. | 0.0034 | b. | 145 | d. | 296 |
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102.
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A substance that slows down a chemical process is called what?
a. | exothermic | c. | inhibitor | b. | endothermic | d. | catalyst |
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103.
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What happens to the rate of a reaction if the temperature is lowered?
a. | it speeds up | c. | it stays the same | b. | it slows down |
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104.
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What is the minimum energy required for an effective collision called?
a. | joule | c. | kinetic energy | b. | calorie | d. | activation
energy |
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105.
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What is the primary reason that an increase in temperature results in an
increase in reaction rates?
a. | it has greater potential energy | c. | there are less
calories | b. | it has greater kinetic energy | d. | the molecules hit each other
less |
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106.
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To react, what must gas particles do?
a. | bounce off each other | c. | collide with opposing orientation
| b. | collide with the correct orientation | d. | get close to each
other |
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107.
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To slow down the rate of reaction, what would you do?
a. | increase the concentration of the reactants | c. | lower the
temperature | b. | increase the surface area of the reactants | d. | adding a
catalyst |
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108.
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A 50.6 g sample of iron metal is heated from 19.7°C to 24.3°C. How
many joules of heat will be absorbed if the specific heat of iron is 0.4494 J/g°C?
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109.
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A sample of an unknown metal has a mass of 120.7 g. As the sample cools from
90.5°C to 25.7°C it releases 7020 J of energy. What is the specific heat of the
sample?
a. | 1.11 | c. | 0.898 | b. | 3769 | d. | 0.000265 |
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110.
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A silver bar with a mass of 250.0 g is heated from 22.0°C to 68.5°C.
How much heat does the silver bar absorb if the specific heat of silver is 0.235 J/g°C.
a. | 2731 | c. | 0.0437 | b. | 0.000366 | d. | 22.88 |
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111.
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If the temperature of 34.4 g of ethanol is heated from 25.0°C to
78.8°C, how much heat has been absorbed by the ethanol of the specific heat of ethanol is
2.44J/g°C?
a. | 19.4 | c. | 0.000145 | b. | 0.0515 | d. | 4516 |
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112.
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Reactions that occur when more energy is released in the forming of new bonds
than is required to break bonds in the initial reactants is an example of what type of
reaction?
a. | endothermic | c. | specific heat | b. | exothermic | d. | neutralization |
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113.
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What are reactions that release energy into its surroundings known as?
a. | endothermic | c. | specific heat | b. | exothermic | d. | neutralization |
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114.
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The temperature of a sample of iron with a mass of
10.0 g changed from 50.4°C to 25.0°C
with the release of 114 J of heat. What is the specific heat of iron?
a. | 0.449 | c. | 285 | b. | 44.9 | d. | 0.0035 |
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115.
|
What type of energy change is shown in the following
reaction?
Sn + Cl2 ®
SnCl2
ÆH = -325 KJ
a. | endothermic | c. | polythermic | b. | exothermic | d. | multithermic |
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116.
|
Find the percent composition of C12H22O11.
a. | %C = 42.1, %H = 6.5, %O = 51.5 | c. | %C = 3.5, %H = 2.9, %O =
93.6 | b. | %C = 12.0, %H = 1.0, %O = 16.0 | d. | %C = 32.7, %H = 16.5, %O =
12.1 |
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117.
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Find the percent composition of CaC2.
a. | %Ca = 62.5, %C = 37.5 | c. | %Ca = 21.1, %C = 78.9 | b. | %Ca = 16.2, %C =
83.8 | d. | %Ca = 50.0, %C =
50.0 |
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118.
|
Find the percent composition of KClO4.
a. | %K =11.9 , %Cl = 12.1, %O = 76.0 | c. | %K = 28.2, %Cl = 25.6, %O =
46.2 | b. | %K = 52.1, %Cl = 6.9, %O = 41.0 | d. | %K = 8.5, %Cl = 9.7, %O =
81.1 |
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119.
|
Find the percent composition of MgS.
a. | %Mg = 17.6, %S = 82.4 | c. | %Mg = 52.1, %S = 47.9 | b. | %Mg = 11.6, %S =
88.4 | d. | %Mg = 43.1, %S =
56.9 |
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120.
|
Find the percent composition of MgSO4.
a. | %Mg = 20.2, %S = 26.6, %O = 53.2 | c. | %Mg = 25.0, %S = 25.0, %O =
50.0 | b. | %Mg = 11.1, %S = 12.6, %O = 76.3 | d. | %Mg = 18.1, %S = 19.7, %O =
62.2 |
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121.
|
A compound contains 36.1 g calcium and 63.9 g
chlorine. What is the empirical formula of the compound?
a. | CaCl3 | c. | CaCl | b. | Ca2Cl2 | d. | CaCl2 |
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122.
|
A compound is composed of 82.68% mercury, (Hg), and 17.32% nitrogen, (N), and
has an experimental molar mass of 485.20 g/mol. What is the compound's empirical formula?
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123.
|
Determine the empirical formula for a compound that contains 35.98% aluminum and
64.02 % sulfur.
a. | Al3S2 | c. | Al2S3 | b. | AlS | d. | AlS3 |
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124.
|
Find the empirical formula of a compound that is 39.12 % C, 8.76% H, and 52.12%
O.
a. | C3H8O3 | c. | CH2O | b. | CHO | d. | C2H3O2 |
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125.
|
Methane (CH4) contains 75% carbon. What percentage of methane is
hydrogen?
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126.
|
The elemental analysis of a sample of ionic compound gave the following results:
2.82 g Na,
4.35 g Cl, and 7.83 g O. The empirical formula of this compound is:
a. | Na2ClO3 | c. | NaClO4 | b. | NaClO3 | d. | NaCl2O |
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127.
|
What is the empirical formula for a compound that is 27.3 % C and 72.7 % O?
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128.
|
What is the molecular formula of a compound that is
composed of 83.64% tin (Sn) and 16.36% phosphorous (P)? The compound's experimental molar mass
is: 479.98 g/mol.
a. | SnP | c. | SnP4 | b. | Sn4P3 | d. | Sn3P2 |
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129.
|
Which energy difference in the reaction profile
below corresponds to the activation energy for the forward reaction?
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130.
|
What type of solution that contains less solute than it is able to hold at a
given temperature?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | poly satuated |
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131.
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What type of solution that contains more solute than it can hold at a given
temperature?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | poly saturated |
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132.
|
What is the general rule for solubility?
a. | like dissolves unlike | c. | like dissolves like | b. | unlike dissolves unlike | d. | unlike dissolves
like |
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133.
|
If a crystal is added to an aqueous solution and it causes many crystals to come
out of the solution, what type of solution was it originally?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | poly saturated |
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134.
|
What term refers to the ease with which an acid or base forms ions in
solution?
a. | pH | c. | base | b. | acid | d. | strength |
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135.
|
What type of solution contains more hydrogen ions than it does hydroxide
ions?
a. | acid | c. | neutral | b. | base | d. | amphoteric |
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136.
|
What will increase the rate of reaction?
a. | lower the temperature | c. | stir | b. | decreast the surface area | d. | grind up the
solvent |
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137.
|
What will happen to the rate of reaction if the surface area of reactants is
increased?
a. | speed up | c. | remains constant | b. | slow down | d. | unable to tell with this
information |
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138.
|
What is the coefficient that belongs in front of oxygen in the equation?
____C3H8 + ___O2 ®
____CO2 + ___H2O
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139.
|
What is the coefficient that belongs in front of water in the equation?
____C3H8 + ___O2 ®
____CO2 + ___H2O
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140.
|
What are the coefficients to correctly balance the formula
equation?
Al2(SO4)3 + KOH à Al(OH)3 +
K2SO4
a. | 2,3,3,2 | c. | 1,6,2,3 | b. | 3,2,3,2 | d. | 2,6,3,1 |
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141.
|
What are the coefficients to correctly balance the formula equation?
Cr + Fe(NO3)2 à
Fe + Cr(NO3)3
a. | 2,3,3,2 | c. | 3,2,2,3 | b. | 3,2,3,2 | d. | 1,3,3,1 |
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142.
|
The following reaction : Cr +
Fe(NO3)2 à Fe +
Cr(NO3)3, can be classified as what type of
reaction?
a. | synthesis | c. | single replacement | b. | decomposition | d. | double
replacement |
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143.
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What type of reaction is this & why?
a. | endothermic - energy is released | c. | exothermic - energy is
released | b. | endothermic - energy is absorbed | d. | exothermic - energy is
absorbed |
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144.
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What type of reaction is this & why?
a. | endothermic - absorbs heat | c. | exothermic - absorbs
heat | b. | endothermic - releases heat | d. | exothermic - releases heat |
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145.
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What type of reactions occurs when more energy is required to break
existing bonds in reactants than is released when new bonds form in the products?
a. | endothermic | c. | poly thermic | b. | exothermic | d. | multi thermic |
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146.
|
What is the molarity of a solution made by dissolving 34.0 g of sodium chloride
(NaCl) in enough water to make 500 mL of solution?
a. | 0.068 | c. | 2.32 | b. | 68 | d. | 0.00232 |
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147.
|
Calculate the molarity of a water solution of KCl, given that 2.50 L of the
solution contains 350 g of KCl.
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148.
|
What would the final volume of a solution be if 25.0 mL of a 1.0 M stock
solution is diluted to
0.50 M?
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149.
|
What is the molarity of a solution containing 9.0 moles of a solute in 500.0 mL
of solution?
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150.
|
What would the final volume of a solution be if 6.0 mL of a 0.050 M stock
solution is diluted to
0.020 M?
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151.
|
If 40.0 ml of a 0.400 M solution of HCl is diluted to 50.0 ml, what will the
final molarity be?
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152.
|
What is the percentage of chromium in BaCrO4?
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153.
|
What is the percentage of barium in BaCrO4?
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154.
|
What is the percentage of oxygen in BaCrO4?
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155.
|
What is the percentage of carbon in C7H16?
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156.
|
Find the empirical formula of a compound that is
65.45 % C, 5.45% H, and 29.09% O.
a. | CHO | c. | C3H3O | b. | C2H2O | d. | CH2O |
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157.
|
Find the empirical formula of a compound that is 53.5 g C, 15.7 g H, 31.1 g
N.
a. | CHN | c. | C3H8N2 | b. | C2H5N | d. | C2H7N |
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158.
|
A colorless liquid composed of 46.68% N and 53.32 % O has a molar mass of 60.01
g/mol. Find the molecular formula.
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159.
|
The specific heat of ethanol is 2.44 J/g°C. How
many joules of energy are required to heat 50.0 g of ethanol from -20.0°C to 68.0°C?
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160.
|
How much heat does it take to warm 16.0 g of pure water from 90°C to 100 °C? The specific heat of water is
4.18 J/g°C.
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161.
|
How much heat does it take to warm 50.00 g of pure water from 20.00°C to 80.00 °C? The specific heat of water
is 4.180 J/g°C.
a. | 862 | c. | 12540 | b. | 1153 | d. | 20685 |
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162.
|
If the temperature of 56.2 g of ethanol increases from 75.1o C to
89.3o C, how much heat has been absorbed by the ethanol? (The specific heat of
ethanol is 2.44 J/g- oC).
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163.
|
The temperature of a sample of water increases from 20.0°C to 46.6°C as it absorbs 5650 J of heat.
What is the mass of the sample? The specific heat of water is 4.18 J/g°C.
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