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Chemistry Study Guide # 1-167



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: 2H2O ® 2H2 + O2?
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.
a.
true
b.
false
 

 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
 
 
nar001-1.jpg
 

 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?
a.
25
c.
100
b.
70
d.
50
 

 17. 

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

 18. 

According to the graph above, at what temperature is the solubility of KBr the same as KNO3?
a.
80
c.
160
b.
50
d.
70
 

 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?
a.
50
c.
30
b.
75
d.
90
 
 
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 CaClmade 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
 

 28. 

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
 

 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 ___.
a.
strong
c.
pH
b.
weak
d.
pOH
 

 34. 

The substances produced when KOH neutralizes HCl are
a.
KH + ClOH
c.
KClH + OH
b.
KCl + H2O
d.
HOH + KCl2
 

 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.
H2O
c.
NaOH
b.
CH4
d.
HCH3COO
 

 37. 

The formula for the products between sodium hydroxide and sulfuric acid are ___.
a.
NaSO4 + H2O
c.
NaS2 + H2O
b.
Na2SO4 + H2O
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 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?
a.
2.2
c.
502
b.
4.1
d.
0.0020
 

 45. 

   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
 

 46. 

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
 

 47. 

   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
 

 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 (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
a.
2430
c.
143
b.
4870
d.
285
 

 50. 

Calculate the number of moles in 250.0g of potassium chlorate (KClO3).
a.
3.35
c.
8.25
b.
2.76
d.
2.04
 

 51. 

Determine the molar mass of KC2H3O2.
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 AgNO3, determine the number of formula units.
a.
0.0191
c.
1.96 x 1024
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 H2O.
                              C4H6  +  O2  ®  CO2 +  H2O
a.
3
c.
2
b.
6
d.
11
 

 55. 

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
 

 56. 

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
 

 57. 

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
 

 58. 

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
 

 59. 

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
 

 60. 

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
 

 61. 

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
a.
9
c.
0.33
b.
1
d.
0.11
 

 62. 

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
 

 63. 

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
 

 64. 

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
 

 65. 

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
 

 66. 

What is the coefficient that belongs in front of carbon dioxide in the equation?
____C3H8 + ___O2 ® ____CO2 + ___H2O
a.
3
c.
4
b.
6
d.
5
 

 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?
      AgNO3(aq)  +    NaCl (aq) ®     AgCl(s)  +  NaNO3(aq)
a.
synthesis
c.
single replacement
b.
decomposition
d.
double replacement
 

 69. 

What is the formula mass of (NH4)3PO4?
a.
121.1
c.
144.07
b.
149.12
d.
153.20
 

 70. 

The molar mass of CO2 is 44 g/mol.  How many moles are present in 110 g?                     
a.
2.50
c.
8.62
b.
4840
d.
1.5
 

 71. 

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
 

 72. 

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
 

 73. 

What type of reaction is 2Hg + O2 ® 2HgO?
a.
single replacement
c.
synthesis
b.
double replacement
d.
decomposition
 

 74. 

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
 

 75. 

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
 

 76. 

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
 

 77. 

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)
a.
9.44
c.
2.36
b.
1.18
d.
4.72
 

 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?
a.
331
c.
595
b.
943
d.
509
 

 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?
a.
812
c.
1520
b.
711
d.
760
 

 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?
a.
1850
c.
702
b.
296
d.
653
 

 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?
a.
699
c.
463
b.
1204
d.
231
 

 82. 

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?
a.
0
c.
1.44
b.
0.696
d.
16.5
 

 83. 

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?
a.
0
c.
0.0959
b.
10.4
d.
17.6
 

 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?
a.
1.33
c.
0.55
b.
1.81
d.
0.75
 

 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 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?
a.
319
c.
24.8
b.
45.9
d.
86.5
 

 89. 

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
 

 90. 

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?
a.
96.2
c.
71
b.
0.010
d.
0.014
 

 91. 

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?
a.
110
c.
167
b.
0.009
d.
0.006
 

 92. 

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a.
128
c.
78.1
b.
7.81
d.
12.8
 

 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?
a.
10
c.
64.6
b.
0.1
d.
0.15
 

 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?
a.
0.32
c.
5.25
b.
3.12
d.
0.19
 

 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 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?
a.
97
c.
45.8
b.
0.01
d.
0.022
 

 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
 

 102. 

A substance that slows down a chemical process is called what?
a.
exothermic
c.
inhibitor
b.
endothermic
d.
catalyst
 

 103. 

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
 

 104. 

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

 105. 

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
 

 106. 

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
 

 107. 

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
 

 108. 

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?
a.
105
c.
0.0409
b.
572
d.
517
 

 109. 

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
 

 110. 

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
 

 111. 

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
 

 112. 

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
 

 113. 

What are reactions that release energy into its surroundings known as?
a.
endothermic
c.
specific heat
b.
exothermic
d.
neutralization
 

 114. 

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
 

 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
 

 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
 

 117. 

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
 

 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
 

 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
 

 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
 

 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
 

 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?
a.
HgN3
c.
HgN
b.
Hg2N6
d.
HgN2
 

 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
 

 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
 

 125. 

Methane (CH4) contains 75% carbon. What percentage of methane is hydrogen?
a.
17
c.
25
b.
63
d.
34
 

 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
 

 127. 

What is the empirical formula for a compound that is 27.3 % C and 72.7 % O?
a.
CO3
c.
CO2
b.
CO
d.
C2O
 

 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
 
 
nar003-1.jpg
 

 129. 

Which energy difference in the reaction profile below corresponds to the activation energy for the forward reaction?
a.
w
c.
y
b.
x
d.
z
 

 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
 

 131. 

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
 

 132. 

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

 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
 

 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
 

 135. 

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

 136. 

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

 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
 

 138. 

What is the coefficient that belongs in front of oxygen in the equation? 
____C3H8 + ___O2 ® ____CO2 + ___H2O 
a.
1
c.
3
b.
5
d.
4
 

 139. 

What is the coefficient that belongs in front of water in the equation? 
____C3H8 + ___O2 ® ____CO2 + ___H2O
a.
1
c.
3
b.
5
d.
4
 

 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
 

 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
 

 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
 
 
nar004-1.jpg
 

 143. 

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
 
 
nar005-1.jpg
 

 144. 

What type of reaction is this & why?
a.
endothermic - absorbs heat
c.
exothermic - absorbs heat
b.
endothermic - releases heat
d.
exothermic - releases heat
 

 145. 

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
 

 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
 

 147. 

Calculate the molarity of a water solution of KCl, given that 2.50 L of the solution contains 350 g of KCl.
a.
140
c.
4.69
b.
0.007
d.
1.88
 

 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?
a.
50
c.
25
b.
0.02
d.
0.01
 

 149. 

What is the molarity of a solution containing 9.0 moles of a solute in 500.0 mL of solution?
a.
0.018
c.
0.1
b.
18
d.
5
 

 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?
a.
2.4
c.
0.067
b.
0.417
d.
15
 

 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?
a.
0.32
c.
0.50
b.
3.13
d.
2.00
 

 152. 

What is the percentage of chromium in BaCrO4?
a.
20.5
c.
11.6
b.
45.8
d.
85.1
 

 153. 

What is the percentage of barium in BaCrO4?
a.
20.7
c.
54.2
b.
13.8
d.
11.6
 

 154. 

What is the percentage of oxygen in BaCrO4?
a.
6.3
c.
87.2
b.
25.3
d.
11.8
 

 155. 

What is the percentage of carbon in C7H16?
a.
83.8
c.
22.8
b.
16.2
d.
75.4
 

 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
 

 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
 

 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.
a.
NO
c.
N2O2
b.
N2O
d.
NO2
 

 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?
a.
10736
c.
567
b.
1803
d.
2468
 

 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.
a.
1950
c.
8452
b.
669
d.
124
 

 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
 

 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).
a.
1947
c.
2258
b.
863
d.
75
 

 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.
a.
168.2
c.
11.7
b.
95
d.
50.8
 



 
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