Chemical Reactions
1. In a balanced chemical reaction equation, the coefficients can be interpreted
as the number of
A. particles only.
B. moles only.
C. molecules only.
D. particles, moles or molecules.
2. In a balanced chemical reaction equation, the coefficients can be interpreted
as the number of
A. grams.
B. moles.
C. joules.
D. litres of gas.
3. S8 + O2 ----> SO2
When the above reaction is balanced, the coefficients from left to right are
A. 0, 8 ---> 0
B. 0, 8 ---> 8
C. 1, 8 ---> 2
D. 1, 8 ---> 8
4. C2H5OH + O2 ----> CO2 + H2O
When the above reaction is balanced, the coefficients from left to right are
A. 1, 7 ---> 2, 3
B. 1, 3 ---> 2, 3
C. 2, 14 ---> 4, 3
D. 2, 7 ---> 2 , 3
5. NiCl3 + K2CO3 ----> Ni2(CO3)3 + KCl
When the above reaction is balanced, the coefficients from left to right are
A. 2, 3 ---> 1, 3
B. 2, 3 ---> 2, 3
C. 2, 6 ---> 3, 6
D. 2, 3 ---> 1, 6
6. Magnesium metal reacts at a high temperature in nitrogen gas to produce
magnesium nitride? When this reaction is written and balanced, the coefficients
from left to right are
A. 1,1 ---> 1
B. 6,1 ---> 2
C. 3,1 ---> 1
D. 2,3 ---> 2
7. Copper I sulfide will react with oxygen to produce copper I oxide and
sulfur dioxide. When the above reaction is balanced, the coefficients from
left to right are
A. 1,1 ---> 1,1
B. 1,2 ---> 1,1
C. 2,3 ---> 2,2
D. 4,3 ---> 3,2
8. When hydrogen phosphate reacts with aluminum hydroxide, the products are
water and aluminum phosphate. When this reaction is written and balanced,
the coefficients from left to right are
A. 1,1 ---> 3,1
B. 3,1 ---> 3,1
C. 2,3 ---> 6,2
D. 3,2 ---> 6,3
9. C2H5OH + O2 ----> CO2 + H2O This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
10. CH4+ O2 ----> CO2 + H2O This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
11. A reaction in which a substance combines with oxygen is an example of
A. synthesis.
B. decompostion.
C. combustion.
D. single replacement.
E. double replacement.
12. Which of the following reactions is a combustion reaction?
A. C5H12 + 8 O2 ----> 5 CO2 + 6 H2O
B. 3 K + FeCl3 ---> 3 KCl + Fe
C. 2 KBr ---> 2 K + Br2
D. 3 F2 + N2 ---> 2NF3
E. NaCl(aq) + AgNO3(aq) ---> AgCl(s) + NaNO3(aq)
13. What products are produced in the combustion of hydrocarbons?
A. CO2, SO2
B. H2, CO2
C. H2O, CO2
D. SO3, CO
14. H2O ----> H2 + O2 This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
15. HCl ----> H2 + Cl2 This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
16. A reaction in which a substance breaks down to form simpler substances
is an example of
A. synthesis.
B. decompostion.
C. combustion.
D. single replacement.
E. double replacement.
17. Which of the following reactions is a decomposition reaction?
A. C5H12+ 8 O2 ----> 5 CO2 + 6 H2O
B. 3 K + FeCl3 ---> 3 KCl + Fe
C. 2 KBr ---> 2 K + Br2
D. 3 F2 + N2 ---> 2NF3
E. NaCl(aq) + AgNO3(aq) ---> AgCl(s) + NaNO3(aq)
18. Which type of reaction has the general form AB ----> A + B ?
A. synthesis
B. decomposition
C. single replacement
D. double replacement
19. FeCl3(aq) + NaOH(aq) ----> Fe(OH)3(s) + NaCl(aq) This reaction is
an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
20. NiCl3(aq) + K2CO3(aq) ----> Ni2(CO3)3(s) + KCl(aq) This reaction is
an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
21. A reaction in which a precipitate forms when two solutions are mixed
is an example of
A. synthesis.
B. decompostion.
C. combustion.
D. single replacement.
E. double replacement.
22. Which of the following reactions is a double replacement reaction?
A. C5H12+ 8 O2 ----> 5 CO2 + 6 H2O
B. 3 K + FeCl3 ---> 3 KCl + Fe
C. 2 KBr ---> 2 K + Br2
D. 3 F2 + N2 ---> 2NF3
E. NaCl(aq) + AgNO3(aq) ---> AgCl(s) + NaNO3(aq)
23. Consider the reaction of phosphoric acid and lithium hydroxide:
H3PO4(aq) + 3LiOH(aq) --> Li3PO4(aq) + 3H2O(1)
This reaction can be classified as a:
A. synthesis reaction.
B. decomposition reaction.
C. combustion reaction.
D. double replacement reaction.
24. Which type of reaction has the general form AB + XY ----> AY + XB?
A. synthesis.
B. single replacement.
C. double replacement.
D. combustion.
25. Which of the following represents an endothermic reaction?
A. S(s) + O2(g) ----> SO2(g) Delta H = -297 kJ
B. 2 NO2(g) ----> N2(g) + 2 O2(g) + 33.8 kJ
C. N2(g) + 2 O2(g) + 90.4 kJ ----> 2 NO
D. N2H4(g) + O2(g) ----> N2(g) + 2 H2O(g) + 627.6 kJ
26. Which of the following represents an endothermic reaction?
A. S(s) + O2(g) ----> SO2(g) Delta H = -297 kJ
B. 2 NO2(g) ----> N2(g) + 2 O2(g) + 33.8 kJ
C. 2 NO ----> N2(g) + 2 O2(g) + 90.4 kJ
D. N2(g) + 2 H2O(g) ----> N2H4(g) + O2(g) Delta H = 627.6 kJ
27. Which of the following represents an endothermic reaction?
A. S(s) + O2(g) ----> SO2(g) Delta H = -297 kJ
B. CaCO3(s) ----> CaO(s) + CO2(g) Delta H = 177.7 kJ
C. 2 B5H9(l) + 12 O2(g) ----> 5 B2O3(s) + 9 H2O + 8753 kJ
D. Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g) + 152 kJ
28. Which of the following statements best describes an endothermic reaction?
A. The energy possessed by the products is > the energy possessed by the reactants.
B. The energy possessed by the products is < the energy possessed by the reactants.
C. The energy possessed by the products can be > or < the energy possessed by the reactants.
D. The energy possessed by the products is + to the energy possessed by the reactants.
29. A chemical reaction is termed endothermic if
A. energy is absorbed during the reaction.
B. energy is required to initiate the reaction.
C. the temperature at which the reaction occurs is very high.
D. energy is released during the reaction.
30. A reaction described as endothermic is one that
A. has a negative Delta H.
B. absorbs heat from the surroundings.
C. undergoes an increase in temperature.
D. has an decrease in heat content.
31. A reaction described as endothermic is one that
A. has a positive Delta H.
B. releases heat to the surroundings.
C. undergoes an increase in temperature.
D. has an decrease in heat content.
32. A reaction described as endothermic is one that
A. has a negative Delta H.
B. releases heat to the surroundings.
C. undergoes an decrease in temperature.
D. has an decrease in heat content.
33. Consider the following reaction; N2(g) + 2 O2(g) + 33.8 kJ ----> 2 NO2(g)
This reaction is
A. endothermic and the reactants are more stable than the products.
B. endothermic and the products are more stable than the reactants.
C. exothermic and the products are more stable than the reactants.
D. exothermic and the reactants are more stable than the products.
34. Consider the following reaction; SO2(g) --> S(s) + O2(g) Delta H = +297 kJ
This reaction is
A. endothermic and the products are more stable than the reactants.
B. endothermic and the reactants are more stable than the products.
C. exothermic and the products are more stable than the reactants.
D. exothermic and the reactants are more stable than the products.
35. Consider the following equation;
2 SO2(g) + O2(g) ----> 2 SO3(g) Delta H = -192.8 kJ
If 3.20 grams of sulphur dioxide gas was consumed, the amount of heat
released would be
A. 4.82 kJ
B. 9.64 kJ
C. 19.3 kJ
D. 38.6 kJ
36. For the reaction;
N2H4(l) + 3 O2(g) --> 2 H2O(g) + NO2(g) Delta H = -400. kJ
the energy released when 14.4 grams of H2O(g) is produced is
A. 40.0 kJ
B. 80.0 kJ
C. 120. kJ
D. 160. kJ
37. Given 2 NaOH(s) ----> Na2O(s) + H2O(l) + 168 J
If 21 J of energy are produced by the above reaction, the mass of
NaOH(s) used is
A. 0.25 g
B. 5.0 g
C. 10. g
D. 32 g
38. Given 2 NaOH(s) ----> Na2O(s) + H2O(l) + 168 J
If 21 J of energy are produced by the above reaction, the mass of Na2O(s)
produced is
A. 3.9 g
B. 7.8 g
C. 15.6 g
D. 31.2 g
39. When 1.0 mol nitrogen reacts with 3.0 mol hydrogen to form 2.0 mol of
ammonia the energy released is 92 kJ. How much energy is released if
0.42 mol nitrogen react?
A. 19kJ
B. 39kJ
C. 77kJ
D. 220kJ
40. Given CH4(g) + 2 O2(g) ----> CO2(g) + 2 H2O(g) + 81 kJ
The Delta H of this reaction per mole of H2O(g) is
A. -81 kJ/mol.
B. +81 kJ/mol.
C. +40.5 kJ/mol.
D. -40.5 kJ/mol.
41. Given 2 C4H10(g) + 13 O2(g) --> 8 CO2(g) + 10 H2O(g) + 5744 kJ
The Delta H of this reaction per mole of CO2(g) is
A. -574.4 kJ/mol.
B. -2872 kJ/mol.
C. -718 kJ/mol.
D. -5744 kJ/mol.
42. Given 2 NaOH(s) + 168 J ----> Na2O(s) + H2O(l)
The Delta H of this reaction per mole of NaOH(s) is
A. +168 J/mol.
B. +84 J/mol.
C. -168 J/mol.
D. -84 J/mol.
43. Given 2 SO2(g) + O2(g) ----> 2 SO3(g) + 192.8 kJ
The Delta H of this reaction per mole of SO3(g) is
A. -192.8 J/mol.
B. +192.8 J/mol.
C. -96.4 J/mol.
D. +96.4 J/mol.
44. Given 2 SO3(g) + 192.8 kJ ----> 2 SO2(g) + O2(g)
The Delta H of this reaction per mole of SO3(g) is
A. -192.8 kJ/mol.
B. +192.8 kJ/mol.
C. -96.4 kJ/mol.
D. +96.4 kJ/mol.
45. Given 2 Fe2O3(s) + 573 kJ ----> 4 FeO(s) + O2(g)
The Delta H of this reaction per mole of Fe2O3(s) used is
A. -573 J/mol.
B. +573 J/mol.
C. -286 J/mol.
D. +286 J/mol.
46. When the reaction, N2(g) + 2 O2(g) + 90.4 kJ ----> 2 NO , is rewritten
for one mole of oxygen gas, the Delta H for the reaction is
A. 90.4 kJ
B. 45.2 kJ
C. -90.4 kJ
D. -45.2 kJ
47. Which of the following represents an exothermic reaction?
A. S(s) + O2(g) ----> SO2(g) Delta H = -297 kJ
B. N2(g) + 2 O2(g) + 33.8 kJ ----> 2 NO2(g)
C. N2(g) + 2 O2(g) ----> 2 NO Delta H = 90.4 kJ
D. CaCO3(s) ----> CaO(s) + CO2(g) Delta H = 177.7 kJ
48. Which of the following represents an exothermic reaction?
A. SO2(g) ----> S(s) + O2(g) Delat H = 297 kJ
B. CaCO3(s) + 177.7 kJ ----> CaO(s) + CO2(g)
C. 2 B5H9(l) + 12 O2(g) ----> 5 B2O3 (s) + 9 H2O + 8753 kJ
D. N2(g) + 2 O2(g) + 90.4 kJ ----> 2 NO
49. Which of the following statements best describes an exothermic reaction?
A. The energy possessed by the products is > the energy possessed by the reactants.
B. The energy possessed by the products is < the energy possessed by the reactants.
C. The energy possessed by the products can be > or < the energy possessed by the reactants.
D. The energy possessed by the products is = to the energy possessed by the reactants.
50. A chemical reaction is termed exothermic if
A. energy is absorbed during the reaction.
B. energy is required to initiate the reaction.
C. the temperature at which the reaction occurs is very high.
D. energy is released during the reaction.
51. Any reaction that releases energy is called a(n)
A. exothermic reaction.
B. combustion reaction.
C. water-forming reaction.
D. endothermic reaction.
52. Which one of the following statements is true about an exothermic reaction?
A. It is accompanied by a decrease in enthalpy.
B. It causes a reduction in the temperature of the system.
C. It requires more energy than it releases.
D. It has products with a higher heat content.
53. Consider the following reaction;
N2H4(g) + O2(g) ----> N2(g) + 2 H2O(g) + 627.6 kJ
This reaction is
A. endothermic and the reactants are more stable than the products.
B. endothermic and the products are more stable than the reactants.
C. exothermic and the reactants are more stable than the products.
D. exothermic and the products are more stable than the reactants.
54. Consider the following reaction;
Na2CO3(s) + 2HCl(aq) ---> 2NaCl(aq) + CO2(g) + H2O(g) + 27.7 kJ
This reaction is
A. endothermic and the reactants have more energy than the products.
B. endothermic and the products have more energy than the reactants.
C. exothermic and the reactants have more energy than the products.
D. exothermic and the products have more energy than the reactants.
55. Consider the following reaction;
MgCO3(s) + 2HCl(aq) ---> 2MgCl2(aq) + CO2(g) + H2O(g) Delta H = -23.4 kJ
This reaction is
A. endothermic and the reactants have less energy than the products.
B. endothermic and the products have less energy than the reactants.
C. exothermic and the reactants have less energy than the products.
D. exothermic and the products have less energy than the reactants.
56. 12 moles of aluminum and 30 moles HCl are combined and react
according to the equation
2 A1 + 6 HCl --> 2 AlCl3 + 3 H2.
One of the reactants is totally consumed. How much of the other
reactant remains unreacted?
A. 2 mol
B. 4 mol
C. 5 mol
D. 6 mol
E. 8 mol
57. If 3 moles of ethane, C2H6, were to react with 14 moles of oxygen, O2,
according to the equation 2 C2H6(g) + 7O2(g) ---> 4 CO2(g) + 6 H2O(l),
which reactant would be in excess?
A. ethane
B. oxygen
C. carbon dioxide
D. water
E. none of the above since the reactants are in the correct ratio
58. How many grams of ammonia is produced when 7.0 g of nitrogen gas is reacted
according to the following equation? 3 H2+ N2 ----> 2 NH3 3 H2+ N2 ----> 2 NH3
A. 2.1 g
B. 4.2 g
C. 8.5 g
D. 17 g
E. 34 g
59. How many grams of copper (II) chloride is needed to react with 14.0 g of iron,
according to the following equation? 3 CuCl2 + 2 Fe ----> 3 Cu + 2 FeCl3 3 CuCl2 + 2 Fe ----> 3 Cu + 2 FeCl3
A. 50.6 g
B. 33.6 g
C. 25.2 g
D. 12.6 g
E. 6.3 g
60. Consider the following balanced equation.
2 NaOH(s) + CO2(g) ---> Na2CO3(s) + H2O(l)
Assuming that there is an excess of carbon dioxide, what is the mass of sodium
hydroxide that is needed to produce 35.0 g of sodium carbonate?
A. 70.0 g
B. 26.4 g
C. 13.2 g
D. 6.6 g
E. 40.0 g
61. Consider the following balanced equation.
SiO2(s) + 4 HF(g) ---> SiF4(s) + 2 H2O(l)
How many grams of SiF4 are produced from the reaction of 6.72 L of HF at STP?
A. 31.2 g
B. 124.9 g
C. 0.71 g
D. 34.9 g
E. 7.81 g
62. Consider the following balanced equation.
SiO2(s) + 4 HF(g) ---> SiF4(s) + 2 H2O(l)
How many litres of HF at STP, are required to produce 31.2 g of SiF4?
A. 26.9 L
B. 29.4 L
C. 6.71 L
D. 1.68 L
E. 31.2 L
63. The mole ratio of hydrogen gas to sulfur in the equation H2(g) + S(s) ---> H2S(g) is:
A. 1 to 1
B. 2 to 1
C. 4 to 1
D. 16 to 1
64. When the reaction,
Al2(SO4)3 + CaCl2 ---> AlCl3 + CaSO4
is balanced, using simplest whole numbers, the quantity of calcium sulfate produced is
A. 1 mol.
B. 2 mol.
C. 3 mol.
D. 6 mol.
65. When the reaction,
Al2(SO4)3 + CaCl2 ---> AlCl3 + CaSO4
is balanced, using simplest whole numbers, the quantity of aluminum chloride produced is
A. 1 mol.
B. 2 mol.
C. 3 mol.
D. 6 mol.
E. 12 mol.
66. When the reaction,
Al2(SO4)3 + CaCl2 ---> AlCl3 + CaSO4 is balanced, using simplest whole numbers,
the true statement is......
A. 1 mol of Al2(SO4)3 will produce 3 mol of AlCl3.
B. 2 mol of Al2(SO4)3 will produce 6 mol of AlCl3.
C. 3 mol of Al2(SO4)3 will produce 3 mol of AlCl3.
D. 2 mol of Al2(SO4)3 will produce 4 mol of AlCl3.
67. When the reaction,
Al2(SO4)3 + CaCl2 ---> AlCl3 + CaSO4 is balanced, using simplest whole numbers, the true statement is......
A. 2 mol of CaCl2 will produce 3 mol of AlCl3.
B. 2 mol of CaCl2 will produce 6 mol of AlCl3.
C. 3 mol of CaCl2 will produce 2 mol of AlCl3.
D. 2 mol of CaCl2 will produce 4 mol of AlCl3.
68. When the reaction,
Fe(NO3)3 + Na2S ---> NaNO3 + Fe2S3 is balanced, using simplest whole numbers,
the true statement is......
A. 4 mol of Fe(NO3)3 will produce 4 mol of Fe2S3.
B. 2 mol of Fe(NO3)3 will produce 4 mol of Fe2S3.
C. 3 mol of Na2S will produce 2 mol of Fe2S3.
D. 6 mol of Na2S will produce 2 mol of Fe2S3.
69. Consider the balanced equation: 2 H2(g) + O2(g) ---> 2 H2O(l)
The INCORRECT statement concerning this reaction is.....
A. 2 molecules of hydrogen react with 1 molecule of oxygen to produce 2 molecules of water.
B. 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.
C. 2 grams of hydrogen react with 1 gram of oxygen to produce 2 grams of water.
D. None of the other options since all are correct.
70. Consider the balanced equation: 2 H2(g) + O2(g) ---> 2 H2O(l)
The INCORRECT statement concerning this reaction is.....
A. 3 molecules of reactants produces 2 molecules of product.
B. 3 moles of reactants produces 2 moles of product.
C. 3 grams of reactants produces 2 grams of product.
D. None of the other options since all are correct.
71. Consider the balanced equation: P4O10 + 6 H2O ---> 4 H3PO4 + heat
The INCORRECT statement concerning this reaction is.....
A. 2 moles of P4O10 will reactant with 12 moles of water.
B. 7 moles of reactants produces 4 moles of product.
C. the quantity of matter reacted will determine the quantity of matter produced.
D. 3 mol of substance has been converted to energy.
72. Given the following balanced equation:
3 Zn + 2 MoO3 ---> Mo2O3 + 3 ZnO
If 4.5 moles of zinc are consumed, how many moles of MoO3 are consumed?
A. 4.5 mol
B. 6.8 mol
C. 3.0 mol
D. 9.0 mol
E. 1.5 mol
73. Given the following balanced equation:
3 Zn + 2 MoO3 ---> Mo2O3 + 3 ZnO
If 4.5 moles of zinc are consumed, how many moles of Mo2O3 are produced?
A. 13.5 mol
B. 6.75 mol
C. 3.0 mol
D. 9.0 mol
E. 1.5 mol
74. Given the following balanced equation:
3 Zn + 2 MoO3 ---> Mo2O3 + 3 ZnO
If 6.5 moles of zinc are consumed, how many moles of MoO3 are consumed?
A. 9.75 mol
B. 4.3 mol
C. 2.2 mol
D. 13.0 mol
E. 6.5 mol
75. Given the following balanced equation:
C6H6 + 7.5 O2 ---> 6 CO2 + 3 H2O
If 10.5 moles of C6H6 are consumed, how many moles of O2 are consumed?
A. 78.8 mol
B. 39.4 mol
C. 10.5 mol
D. 1.40 mol
E. 157 mol
76. 12.00 moles of aluminum reacts with hydrochloric acid according to the equation:
2 Al + 6 HCl --> 2 AlCl3 + 3 H2
How many grams of HCl react?
A. 146.0 g
B. 438.0 g
C. 1314 g
D. 1.313 g
E. 4.370 g
77. Two products formed from the burning of a salt are magnesium oxide
and sulfur dioxide. The salt must have contained
A. sulfur and oxygen.
B. oxygen and magnesium.
C. sulfur and hydrogen.
D. magnesium and sulfur.
78. Two products formed from the burning of a compound are carbon dioxide
and sulfur dioxide. The compound
A. must have contained sulfur and oxygen.
B. could contain any metal and non-metal.
C. must have contained sulfur and carbon.
D. must have contained carbon and oxygen.
79. The formula for the missing reactant is
Na2CO3 + ? ----> H2CO3 + Na3PO4
A. 2 HPO4
B. H2PO4
C. H3PO4
D. H4PO4
80. When the reaction in # 79 is balanced, the coefficients from left to right are
A. 3, 1 ---> 3, 2
B. 3, 2 ---> 3, 2
C. 2, 3 ---> 2, 3
D. 2, 3 ---> 1, 3
81. The formula for the missing product is
CaS + Al(OH)3 ----> Al2S3 + ?
A. 2 CaOH
B. CaO2H2
C. CaOH2
D. Ca(OH)2
82. When the reaction in #81 is balanced, the coefficients from left to right are
A. 3, 1 ---> 3, 2
B. 3, 2 ---> 3, 2
C. 2, 3 ---> 1, 3
D. 3, 2 ---> 1, 3
83. HCl + Mg ----> H2 + MgCl2 This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
84. CuCl2 + Fe ----> Cu + FeCl3 This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
85. A reaction in which one element takes the place of another in a
compound is an example of
A. synthesis.
B. decompostion.
C. combustion.
D. single replacement.
E. double replacement.
86. Which of the following reactions is a single replacement reaction
A. C5H12 + 8 O2 ----> 5 CO2 + 6 H2O
B. 3 K + FeCl3 ---> 3 KCl + Fe
C. 2 KBr ---> 2 K + Br2
D. 3 F2 + N2 ---> 2NF3
E. NaCl + AgNO3 ---> AgCl + NaNO3
87. In which of the following reactions is an atom changed into an ion?
A. C5H12 + 8 O2 ----> 5 CO2 + 6 H2O
B. 2NF3 ---> 3 F2 + N2
C. NaCl + AgNO3 ---> AgCl + NaNO3
D. 3 Li + FeCl3 ---> 3 LiCl + Fe
88. In which of the following reactions is an atom changed into an ion?
A. 2 C6H14 + 19 O2 ----> 12 CO2 + 14 H2O
B. 3 K2S + 2 FeCl3 ---> 6 KCl + Fe2S3
C. NaCl + AgNO3 ---> AgCl + NaNO3
D. F2 + Mg ---> MgF2
89. Consider the reaction of iron and copper sulphate:
Fe(s) + CuSO4(aq) ---> FeSO4(aq) + Cu(s)
This reaction can be classified as a
A. synthesis reaction.
B. decomposition reaction.
C. combustion reaction.
D. single replacement reaction.
E. double replacement reaction
90. Which of the following reactions is a single replacement?
A. 2Mg + O2 ---> 2MgO
B. Fe + CuSO4 ---> FeSO4 + Cu
C. HCl + NaOH ---> NaCl + H2O
D. CaCO3 ---> CaO + CO2
91. Which type of reaction has the general form A + BC ----> AC + B?
A. synthesis
B. single replacement
C. double replacement
D. combustion
92. The chemical joining of two or more elements to form a compound is known as
A. synthesis.
B. decomposition.
C. double replacement.
D. combustion.
93. H2 + N2 ----> NH3 This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
94. H2 + Cl2 ----> HCl This reaction is an example of
A. synthesis
B. decompostion
C. combustion
D. single replacement
E. double replacement
95. A reaction in which simpler substances combine to form a more complex
substance is an example of
A. synthesis.
B. decompostion.
C. combustion.
D. single replacement.
E. double replacement.
96. Which of the following reactions is a synthesis reaction?
A. 3 K + FeCl3 ---> 3 KCl + Fe
B. RbCl + AgNO3 ---> AgCl + RbNO3
C. 2 KBr ---> 2 K + Br2
D. 3 F2 + N2 ---> 2NF3
E. C5H12+ 8 O2 ----> 5 CO2 + 6 H2O
97. Consider the reaction of barium and oxygen gas:
Ba(s) + O2(g) BaO2(s) + Energy
This reaction can be classified as a
A. synthesis reaction.
B. decomposition reaction.
C. water-forming reaction.
D. single replacement.
E. double replacement.
98. Which type of reaction has the general form A + B ----> AB?
A. synthesis
B. decomposition
C. single replacement
D. double replacement
99. Which of the following statements about chemical reactions is FALSE?
A. Atoms or ions are rearranged to produce new substances.
B. Energy is either released or absorbed.
C. Mass is conserved.
D. New atoms are created.
100. Which of the following statements about chemical reactions is FALSE?
A. Atoms or ions are rearranged.
B. Energy is either released or absorbed.
C. Mass is destroyed.
D. Atoms are conserved.
101. Which of the following statements about chemical reactions is FALSE?
A. Atoms can be rearranged to produce molecules.
B. Energy is either created or destroyed.
C. Mass is conserved.
D. Molecules can be decomposed into atoms.
102. Which of the following statements about chemical reactions is TRUE?
A. The mass of the products can be greater than the mass of the reactants.
B. The mass of the products can be less than the mass of the reactants.
C. The mass of the products must equal the mass of the reactants.
D. All of the other options could be true.
103. Which of the following statements about chemical reactions is TRUE?
A. The reaction may produce new molecules through rearrangement of the atoms.
B. The mass of the products can be less than the mass of the reactants.
C. The number of moles of the products must equal the number of moles of the reactants.
D. The number of molecules in the products must equal the number of molecules of the reactants.
104. Which of the following statements about chemical reactions is TRUE?
A. The reaction may produce new atoms through atomic rearrangement.
B. The number of atoms in the products must equal the number of atoms in the reactants.
C. The number of moles of the products must equal the number of moles of the reactants.
D. The number of molecules in the products must equal the number of molecules of the reactants.
105. Which of the following statements about chemical reactions is FALSE?
A. The energy possessed by the products can be greater than the energy possessed by the reactants.
B. The energy possessed by the products can be less than the energy possessed by the reactants.
C. The energy possessed by the products can be greater or less than the energy possessed by the reactants.
D. Energy is not involved in chemical reactions.
106. Substances written to the left of the arrow in an equation are called
A. coefficients.
B. subscripts.
C. reactants.
D. products.
107. Chemical substances written to the right of the arrow in an equation are called
A. coefficients.
B. subscripts.
C. reactants.
D. products.
108. Numbers written in front of formulas in an equation are called
A. coefficients.
B. subscripts.
C. reactants.
D. products.
109. Numbers written after a symbol in a formula are called
A. coefficients.
B. subscripts.
C. reactants.
D. products.
110. Which of the following statements about chemical reactions is TRUE?
A. Atoms are rearranged to form new atoms.
B. Energy is either released or absorbed.
C. Mass is destroyed if one of the products is a gas.
D. Moles of reactant equals moles of products.