Chemistry 11: Chemical Reactions

1. Difference and examples of:

Qualitative

Quantatitive

2. What is a physical change? Examples.

3. What are chemical properties of matter? Examples?

4. What is a chemical change? Examples.

5. How do most chemical reactions take place?

6. The statement “methanol boils at 780C” is an example of a:

physical property
physical change
chemical property
chemical change

7. The statement “phosphorus ignites in contact with air” is an example of a:

physical property
physical change
chemical property
chemical change

8. The statement “oxygen supports combustion” is an example of a:

physical property
physical change
chemical property
chemical change

9. The statement “melting ice” is an example of a:

physical property
physical change
chemical property
chemical change

10. During a chemical reaction, at least one new substance is formed.

What is a reactant?

What is a product?

11.

Write a chemical equation for the following reaction: “iron filings react with sulphuric acid to produce hydrogen and iron(II) sulphate

12. Follow these steps when writing a chemical equation:

What are the steps for writing a chemical equation?

13. What is the law of conservation of mass?

What is an explanation when a reaction appears to gain or lose mass?

14. What are the four main types of chemical reactions?

15. What is a synthesis reaction? What can they also be called?

How is a compound formed?

13. What is the law of conservation of mass?

What is the explanation for when a reaction appears to have gained or lose mass?

14. What are the four different types of chemical reactions?

15. What is a synthesis reactions? (Example) What are alternative names for this reaction?

How is a new compound formed?

16. What is a Decomposition Reaction? (Example)

17. What is a single displacement reaction? (Example)

18. What is a Double Displacement Reaction? (Example)

19. What is a precipitate?

20. What type of reaction is the following?
2Mg + O2 -> 2MgO

synthesis
decomposition
single displacement
double displacement

21. What type of reaction is the following?
2HCl + Na2CO3 -> 2NaCl + H2CO3

synthesis
decomposition
single displacement
double displacement

22. State the missing reactant in the following single displacement reaction.
Blank + 3Fe -> Fe3O4 + 4H2

23. State the missing reactant in the following decomposition reaction.
4HNO3, -> blank + 2H2O + O2

24. During chemical reactions, there is almost always some type of absorption or release of energy.

List some examples that energy can be in the form of?

25. What is an endothermic reaction?

The symbol Q in a chemical equation is a generic representation for energy in the form of heat. Where is it placed in chemical equation for endothermic reactions?
(Examples)

26. What are exothermic reactions?

The symbol Q in a chemical equation is a generic representation for energy in the form of heat. Where is it placed in chemical equation for exothermic reactions?
(Examples)

27. Why do animals require oxygen?

What does oxygen require?

28. What is the unbalanced chemical equation for respiration?

29. What is the unbalanced chemical equation for photosynthesis?

30. What is oxidation?

Give examples of oxidation

31. When is oxidation considered combustion?

32. When does a combustion reaction occur?

33.

When metals are burned they produce...

34.
When non-metals are burned...

35. When will hydrocarbon combust completely?

36. What is released in a complete combustion?

37. What has rising carbon dioxide gas levels been linked to?

38. When does incomplete combustion take place?

39. Incomplete combustion results in two additional substances being produced:

40. Oxygen gas is formed when two atoms of oxygen bond together.

41. Oxygen gas may participate in chemical reactions as either a reactant or product.

41. Combustion is a chemical reaction that takes place slowly and releases oxygen gas.

42. As long as fuels burn completely, there is no environmental risk or damage.

43.
Carbon monoxide gas is extremely dangerous and difficult to detect.

44. Write the balanced chemical equation for combustion of C7H6O.

45. What is an oxidation reaction?

46. Most metal oxides are _________ that react with water to form ________, and are called ______

47. Non-metal oxides tend to be...

Give a few examples

48. Give a few examples of metal oxides

49. Where is nitrogen dioxide found?

50.
Non-metal oxides react with water to form ___, so they are called ____.

51. Which one of the following oxides is considered to be acidic?

CaO
SrO
CO2
Na2O

52. Copper(II) oxide is more acidic than carbon dioxide.

53. Phosphorus pentoxide is more basic than sulphur trioxide.

54. Molecules that contain an H+ ion, such as HCl and H2SO4, are called _____________. Molecules that contain an OH- ion, such as NaOH and Ba(OH)2 are called _____________.

55. What is a neutralization reaction?

56. What are spectator ions?

57. Some common examples and applications of neutralization are:
acid

58. Will 1 mL of acid neutralize 1 mL of any base

59. How do you dilute an acid or base?

60. If there are H+ ions left over after the neutralization reaction, then the solution is _____

61. If there are OH- ions left over after the neutralization reaction, then the solution is _____

62. What are the products of the following neutralization reaction?

H2SO4 + RbOH -->

63. What did Avagardo state regarding the volume of gases?

64. Avogadro's number

65. one mole contains as many entities as there are ...

66. How many atoms are in 0.5 mol of sodium?

67. How many moles of magnesium are there in 3.01 x 1022 atoms of magnesium?

68. How many moles of tungsten correspond to 5.05 x 10^20 atoms?

69. Formula for molar mass

70. What is molar mass?

71. Calculate the molar mass of Al(NO3)3.

72. What is a hydrate?

73. How do you name a hydrate?

74. Convert 2.5 mol of KClO3 to grams.

75. Calculate how many moles are in 17.0 g of H2O2

76. What is the mass of one molecule of H2O?

77. What is the law of definite proportions/ constant composition

78. Calculate the percentage composition (by mass) of Al2O3.

79. 13.0 g of tin is burned in the presence of oxygen to form 16.5 g of tin (IV) oxide. Which of the following represents the percentage composition of tin by mass in this compound?
33.5%
44.1%
78.8%
85.1%

80. What does the empirical formula indicate?

81. A sample of calcium chloride contains 1.82 g of calcium and 3.23 g of chlorine. What is the empirical formula for the compound?

82. The elemental analysis of an unknown organic compound returns the following data:

%C = 64.6%
%H = 10.8%
%O = 24.6%
What is the empirical formula for this compound?

83. What does the molecular formula indicate?

How is it determined?

84. Hydrogen peroxide is made of 5.03% hydrogen and 79.87% oxygen. Its molar mass is 34.01 g/mol. Find its molecular formula.

85. If 4.04 g of nitrogen combine with 11.46 g of oxygen to produce a compound with a molar mass of 108.0 g/mol, what is the molecular formula of this compound?

86. What does quantitative chemical analysis determine?

87. What is Stoichiometry the study of?

What is an analogy to this?

88. How many moles of product could 10 moles of nitrogen produce?

N2 + 3H2 → 2NH3

89.
How many moles of oxygen are produced by the decomposition of 2.8 mol of potassium chlorate?

2KClO3 → 2KCl + 3O2

90. Calculate the number of moles of silver nitrate that are needed in order to completely react with 7.1 mol of copper.

Cl2 + 2Na --> 2NaCl

91. Propane is a gas that is commonly used in BBQs. Its formula is C3H8. Calculate the mass of water that is produced by the combustion of 13.8 mol of propane.

C3H8 + 5O2 --> 3CO2 + 4H2O

92. How many moles of chlorine are required to react completely with 48.6 g of sodium to produce sodium chloride?

2NA + Cl2 --> 2NaCL

93. Calculate how many grams of ammonia can be produced when 206.9 g of nitrogen reacts with hydrogen.

N2 + 3H2 --> 2NH3

94. What is the theoretical yield?

95. What is the actual yield?

95. What is the period yield?

96. organic chemist reacts 10 g of CH4 with excess Cl2. She obtained 10 g of CH3Cl and some H2.

a) What is the theoretical yield?
b) What is her percentage yield?

2CH4 + Cl2 --> 2CH3Cl + H2

97. 36 g of ethyl ethanoate (CH3CO2C2H5) are obtained from 23 g of ethanol (C2H5OH) using the following equation:

C2H5OH + CH3CO2H --> CH3CO2C2H5 + H2O

What is the % yield?

98. What is the limit reagent/reactant?

What does it mean when a reactant is in excess?

99. Methane, CH4, burns in oxygen to give carbon dioxide and water according to the following equation:

CH4 + 2O2 --> CO2 + 2H2O

In an experiment, a mixture of 0.25 mol of methane is burned in 1.25 mol of oxygen in a sealed steel vessel. Find the limiting reactant.

100. What is the solubility of a substance?

101. The solubility of a substance can be affected by:

102. The rate at which a substance dissolves is affected by: