Multiple Choice Identify the
choice that best completes the statement or answers the question.


1.

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 


2.

A solution that contains all of the solute it can hold at a given temperature is
____.
a.  diluted  c.  supersaturated  b.  saturated  d.  unsaturated 


3.

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 


4.

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. 


5.

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. 


6.

When one element replaces another element in a compound, the reaction is a ____
reaction.
a.  decomposition  c.  single–displacement  b.  double–displacement  d.  synthesis 


7.

A substance that speeds up a chemical reaction without being permanently changed
itself is a(n) ____.
a.  catalyst  c.  inhibitor  b.  coefficient  d.  reactant 


8.

What type of reaction is shown in the following chemical equation:
2H_{2}O ® 2H_{2} + O_{2}?
a.  decomposition  c.  single–displacement  b.  double–displacement  d.  synthesis 


9.

____ change color in the presence of an acid or a base.
a.  Acids  c.  Buffers  b.  Glycerins  d.  Indicators 


10.

Coffee has a pH of about 5. Coffee is ____.
a.  extremely acidic  c.  somewhat acidic  b.  extremely basic  d.  somewhat basic 


11.

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 


12.

Increasing temperature generally increases the solubility of a solute in a
solvent.


13.

In a solution, the substance that is being dissolved is the ____.
a.  gas  c.  solute  b.  liquid  d.  solvent 


14.

If two liquids are soluble in each other, they are said to be _____.
a.  soluble  c.  miscible  b.  insoluble  d.  immiscible 


15.

The substance in a solution that dissolves another substance is called
___.
a.  solute  c.  electrolyte  b.  solvent  d.  nonelectrolyte 





16.

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?


17.

According to the graph above, which salt is more soluble in water KCl or
KBr?


18.

According to the graph above, at what temperature is the solubility of KBr the
same as KNO_{3}?


19.

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 


20.

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 


21.

According to the graph, how many grams of KCl wil form a saturated solution in
100 g of water at 60°C?



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   


22.

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 


23.

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 


24.

A mixture with particles that will settle out if left undisturbed is a(n)
___.
a.  suspension  c.  colloid  b.  emulsion  d.  electrolyte 


25.

A solution in which the solvent is water is called ___.
a.  concentrated  c.  aqueous  b.  dilute  d.  amphoteric 


26.

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} 


27.

Calculate the molarity of a water soluiton of CaCl_{2 }made by
dissolving 612 g of CaCl_{2} in 5.04 L of solution.
a.  1.09 M  c.  0.775 M  b.  22.0 M  d.  1.88 M 


28.

What is the molarity of an aqueous solution containing 40.0 g of glucose
(C_{6}H_{12}O_{6}) in 1.5 L of solution?
a.  27 M  c.  0.22 M  b.  60 M  d.  0.15 M 


29.

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 


30.

____________ 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 


31.

A ___ solution contains more hydroxide ions that it does hydrogen ions.
a.  acidic  c.  neutral  b.  basic  d.  saturated 


32.

Since nitric acid is a ____ acid, it ionizes completely in solution
a.  concentrated  c.  strong  b.  dilute  d.  weak 


33.

The negative logarithm of the hydrogen ion concentration is ___.


34.

The substances produced when KOH neutralizes HCl are
a.  KH + ClOH  c.  KClH + OH  b.  KCl + H_{2}O  d.  HOH +
KCl_{2} 


35.

Which expression represents the pH of a solution?
a.  log [H^{+}]  c.  antilog
[pOH]  b.   log [H^{+}]  d.  antilog
[pOH] 


36.

Which is a strong base?
a.  H_{2}O  c.  NaOH  b.  CH_{4}  d.  HCH_{3}COO 


37.

The formula for the products between sodium hydroxide and sulfuric acid are
___.
a.  NaSO_{4} + H_{2}O  c.  NaS_{2 }+
H_{2}O  b.  Na_{2}SO_{4} + H_{2}O  d.  NaH + SOH 


38.

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 


39.

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 


40.

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 


41.

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 


42.

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 


43.

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 


44.

8 KClO_{3} +
C_{12}H_{22}O_{11} ® 8 KCl
+ 12 CO_{2} + 11 H_{2}O If 3.0 moles of potassium chlorate
are used, how many moles of water would be produced?


45.

8 KClO_{3} +
C_{12}H_{22}O_{11} ® 8 KCl
+ 12 CO_{2} + 11 H_{2}O If 25.0 g of carbon dioxide
are produced, how many grams of sugar (C_{12}H_{22}O_{11}) were used?
a.  0.0473  c.  16.2  b.  21.1  d.  0.0617 


46.

8 KClO_{3} +
C_{12}H_{22}O_{11} ® 8 KCl
+ 12 CO_{2} + 11 H_{2}O How many grams of sugar
(C_{12}H_{22}O_{11}) 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 


47.

8 KClO_{3} +
C_{12}H_{22}O_{11} ®8 KCl +
12 CO_{2} + 11 H_{2}O 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 


48.

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 


49.

Ammonia (NH_{3}) is used to make fertilizer. If you have 2.00 x 10
^{3}g of N_{2} how many grams of ammonia can be
produced?
N_{2} +
3H_{2} à
2NH_{3 }


50.

Calculate the number of moles in 250.0g of potassium chlorate
(KClO_{3}).


51.

Determine the molar mass of KC_{2}H_{3}O_{2}.
a.  68.12  c.  86.14  b.  98.15  d.  82.15 


52.

Determine the number of moles in 25.50 g Ag.
a.  0.236  c.  3.64 x 10^{4}  b.  2750  d.  4.24 


53.

Given 3.25 mol of AgNO_{3}, determine the number of formula
units.
a.  0.0191  c.  1.96 x 10^{24}  b.  5.40 x
10^{24}  d.  52.4 


54.

Given the following combustion reaction of a hydrocarbon, balance the equation
and determine the coefficient of
H_{2}O.
C_{4}H_{6} + O_{2} ®
CO_{2 } + H_{2}O


55.

How many atoms of Cu are in 4.00 moles?
a.  254  c.  2.41 x 10^{24}  b.  0.00393  d.  6.64 x
10^{24} 


56.

How many grams of CCl_{4} are in 4.00 moles? The formula mass of
carbon tetrachloride is 153.8 g/mol.
a.  0.026  c.  2.41 x 10^{24}  b.  615  d.  4.15 x
10^{25} 


57.

How many grams of CH_{3}Br could be made from 10.0 g of CH_{3}OH
and excess PBr_{3}?
3 CH_{3}OH +
PBr_{3} à 3
CH_{3}Br + P(OH)_{3}
a.  23.4  c.  4.27  b.  0.0428  d.  0.234 


58.

How many grams of ZnCl_{2} are produced from 75.00 g of ZnO in the
reaction ZnO + 2HCl ® ZnCl_{2} + H_{2}O ?
a.  44.79  c.  125.6  b.  0.0223  d.  0.00796 


59.

How many hydrogen atoms are there in 1.0 x 10^{2} g of glucose,
C_{6}H_{12}O_{6}?
a.  0.555  c.  3.34 x 10^{23}  b.  4.01 x
10^{24}  d.  2.49 x
10^{25} 


60.

How many moles are in 1.2 X 10^{24} molecules of water?
a.  0.503  c.  7.72 x 10^{47}  b.  1.38 x
10^{48}  d.  1.99 


61.

How many moles of CH_{3}Br could be made from 3.0 moles of
PBr_{3} and excess
CH_{3}OH?
3 CH_{3}OH +
PBr_{3} à 3
CH_{3}Br + P(OH)_{3}


62.

If the pressure exerted by a gas at 25.0^{o} C in a volume of 0.0440 L
is 3.81 atm, how many moles of gas are present? (Hint: R = 0.0821 Latm/molK)
a.  0.00685  c.  12.2  b.  0.0817  d.  146 


63.

In the equation HCl + KOH ® KCl +
H_{2}O, 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 


64.

In the reaction 2Na + Cl_{2} ®
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 


65.

One in a series of reactions that inflates airbags in automobiles is the
decomposition of sodium azide
(NaN_{3}).
2 NaN_{3} (s) ® 2 Na (s)
+ 3 N_{2} (g) Determine
the mass of N_{2} produced if 1.00 x 10^{2} g NaN_{3} is decomposed.
a.  21.5  c.  0.00215  b.  464  d.  64.64 


66.

What is the coefficient that belongs in front of carbon dioxide in the
equation? ____C_{3}H_{8} + ___O_{2} ®
____CO_{2} + ___H_{2}O


67.

What is the correct molar mass of Ca(OH)_{2} ?
a.  74.1  c.  58.11  b.  57.09  d.  60.75 


68.

The
following reaction is an example of which type of reaction?
AgNO_{3(aq)} + NaCl
_{(aq)} ® AgCl_{(s)}
+ NaNO_{3(aq)}
a.  synthesis  c.  single replacement  b.  decomposition  d.  double
replacement 


69.

What is the formula mass of (NH_{4})_{3}PO_{4}?
a.  121.1  c.  144.07  b.  149.12  d.  153.20 


70.

The molar mass of CO_{2} is 44 g/mol. How many moles are present
in 110 g?


71.

The molar mass of H_{2}O 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 


72.

The molar mass of NH_{3} is 17.0 g/mol. How many grams of NH_{3}
are present in 3.50 moles?
a.  59.5  c.  0.210  b.  0.0170  d.  4.85 


73.

What type of reaction is 2Hg + O_{2} ®
2HgO?
a.  single replacement  c.  synthesis  b.  double replacement  d.  decomposition 


74.

What are the coefficients to correctly balance the formula equation
Pb(NO_{3})_{2 (aq)} + KI _{(aq)} ® PbI_{2 (s)} + KNO_{3(aq)}
a.  1 2 1 2  c.  1 4 1 4  b.  2 1 2 1  d.  4 1 4 1 


75.

What are the coefficients to correctly balance the formula equation
AlCl_{3(aq)} + Pb(NO_{3})_{2(aq)} ® PbCl_{2(s)} +
Al(NO_{3})_{3(aq)}
a.  3 2 3 2  c.  1 7 4 2  b.  2 3 3 2  d.  5 1 1 2 


76.

What is the balanced equation when aluminum reacts with
copper(II)sulfate?
a.  Al + CuSO_{4} ® Cu +
AlSO_{4}  c.  4Al + 3Cu_{2}(SO_{4})_{2 }®
6Cu + 2Al_{2}(SO_{4})_{3}  b.  2Al + 3CuSO_{4} ® 3Cu + Al_{2}(SO_{4})_{3}  d.  2Al +
Cu_{2}(SO_{4})_{2} ® 2Cu +
2AlSO_{4} 


77.

What volume of oxygen is needed to completely combust 2.36 L of methane gas
(CH_{4})?
CH_{4 }(g) + 2 O_{2}
(g) ®CO_{2}
(g) + 2 H_{2}O (g)


78.

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?


79.

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?


80.

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?


81.

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?


82.

A sample of ammonia gas occupies a volume of 1.58 L at 22.0^{o} C and a
pressure of 0.983 atm. What volume will the sample occupy at 1.00 atm and 0
^{o}C?


83.

A sample of ammonia gas occupies a volume of 27.4 L at 14.0^{o} C and a
pressure of 1.20 atm. What volume will the sample occupy at 3.00 atm and 0 ^{o}C?


84.

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 


85.

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 


86.

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?


87.

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 


88.

A sample of SO_{2} gas has a volume of 1.16 L at a temperature of
23^{o} C. At what temperature will the gas have a volume of 1.25 L?


89.

A sample of SO_{2} 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 


90.

A student collects 285 mL of O_{2} 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 11.0^{o} C, What is the new pressure of the
gas?


91.

A student collects 355 mL of O_{2} 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 17^{o} C, What is the new pressure of the gas?


92.

Calculate the volume that a 0.323mol sample of a gas will occupy at 265 K and a
pressure of 0.900 atm.


93.

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 


94.

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 


95.

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?


96.

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?


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 


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 


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 


100.

You have 200.0 cm^{3} of nitrogen (IV) oxide at a temperature of 303.0 K
and a pressure of 101.0 kPa. What volume will the NO_{2} occupy at 255.0 kPa and 371.0
K?


101.

You have 422.0 cm^{3} of nitrogen (IV) oxide at a temperature of 295.15
K and a pressure of 101.325 kPa. What volume will the NO_{2} occupy at 155.00 kPa and 317.15
K?
a.  0.0069  c.  0.0034  b.  145  d.  296 


102.

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 


103.

What is the minimum energy required for an effective collision called?
a.  joule  c.  kinetic energy  b.  calorie  d.  activation
energy 


104.

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 


105.

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 


106.

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 


107.

Find the percent composition of C_{12}H_{22}O_{11}.
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 


108.

Find the percent composition of CaC_{2}.
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 


109.

Find the percent composition of KClO_{4}.
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 


110.

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 


111.

Find the percent composition of MgSO_{4}.
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 


112.

A compound contains 36.1 g calcium and 63.9 g
chlorine. What is the empirical formula of the compound?
a.  CaCl_{3}  c.  CaCl  b.  Ca_{2}Cl_{2}  d.  CaCl_{2} 


113.

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?
a.  HgN_{3}  c.  HgN  b.  Hg_{2}N_{6}  d.  HgN_{2} 


114.

Determine the empirical formula for a compound that contains 35.98% aluminum and
64.02 % sulfur.
a.  Al_{3}S_{2}  c.  Al_{2}S_{3}  b.  AlS  d.  AlS_{3} 


115.

Find the empirical formula of a compound that is 39.12 % C, 8.76% H, and 52.12%
O.
a.  C_{3}H_{8}O_{3}  c.  CH_{2}O  b.  CHO  d.  C_{2}H_{3}O_{2} 


116.

Methane (CH_{4}) contains 75% carbon. What percentage of methane is
hydrogen?


117.

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.  Na_{2}ClO_{3}  c.  NaClO_{4}  b.  NaClO_{3}  d.  NaCl_{2}O 


118.

What is the empirical formula for a compound that is 27.3 % C and 72.7 % O?
a.  CO_{3}  c.  CO_{2}  b.  CO  d.  C_{2}O 


119.

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.  SnP_{4}  b.  Sn_{4}P_{3}  d.  Sn_{3}P_{2} 





120.

Which energy difference in the reaction profile
below corresponds to the activation energy for the forward reaction?


121.

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 


122.

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 


123.

What is the general rule for solubility?
a.  like dissolves unlike  c.  like dissolves like  b.  unlike dissolves unlike  d.  unlike dissolves
like 


124.

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 


125.

What term refers to the ease with which an acid or base forms ions in
solution?
a.  pH  c.  base  b.  acid  d.  strength 


126.

What type of solution contains more hydrogen ions than it does hydroxide
ions?
a.  acid  c.  neutral  b.  base  d.  amphoteric 


127.

What will increase the rate of reaction?
a.  lower the temperature  c.  stir  b.  decreast the surface area  d.  grind up the
solvent 


128.

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 


129.

What is the coefficient that belongs in front of oxygen in the equation?
____C_{3}H_{8} + ___O_{2} ®
____CO_{2} + ___H_{2}O


130.

What is the coefficient that belongs in front of water in the equation?
____C_{3}H_{8} + ___O_{2} ®
____CO_{2} + ___H_{2}O


131.

What are the coefficients to correctly balance the formula
equation?
Al_{2}(SO_{4})_{3} + KOH à Al(OH)_{3} +
K_{2}SO_{4}
a.  2,3,3,2  c.  1,6,2,3  b.  3,2,3,2  d.  2,6,3,1 


132.

What are the coefficients to correctly balance the formula equation?
Cr + Fe(NO_{3})_{2 }à
Fe + Cr(NO_{3})_{3}
a.  2,3,3,2  c.  3,2,2,3  b.  3,2,3,2  d.  1,3,3,1 


133.

The following reaction : Cr +
Fe(NO_{3})_{2 }à Fe +
Cr(NO_{3})_{3, }can be classified as what type of
reaction?
a.  synthesis  c.  single replacement  b.  decomposition  d.  double
replacement 


134.

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 


135.

Calculate the molarity of a water solution of KCl, given that 2.50 L of the
solution contains 350 g of KCl.


136.

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?


137.

What is the molarity of a solution containing 9.0 moles of a solute in 500.0 mL
of solution?


138.

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?


139.

If 40.0 ml of a 0.400 M solution of HCl is diluted to 50.0 ml, what will the
final molarity be?


140.

What is the percentage of chromium in BaCrO_{4}?


141.

What is the percentage of barium in BaCrO_{4}?


142.

What is the percentage of oxygen in BaCrO_{4}?


143.

What is the percentage of carbon in C_{7}H_{16}?


144.

Find the empirical formula of a compound that is
65.45 % C, 5.45% H, and 29.09% O.
a.  CHO  c.  C_{3}H_{3}O  b.  C_{2}H_{2}O  d.  CH_{2}O 


145.

Find the empirical formula of a compound that is 53.5 g C, 15.7 g H, 31.1 g
N.
a.  CHN  c.  C_{3}H_{8}N_{2}  b.  C2H_{5}N  d.  C_{2}H_{7}N 


146.

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.
a.  NO  c.  N_{2}O_{2}  b.  N_{2}O  d.  NO_{2} 
