Chemistry Worksheets

Name: ______

Period: ______

Teacher: ______

Table of Contents

PageDescription

3 Scientific Notation

6Significant Figures

9Density

10States of Matter

11Protons, Neutrons and Electrons

12Periodic Table and OxidationStates

13Electron Configurations

15 Types of Solids

16Naming Ionic Compounds

18Naming Covalent Compounds

19Compounds Naming and Formula Writing

21 Finding Heats of Reaction

22 Calorimetry

23 Lewis Structures

26Word Equations

27Writing Complete Equations

28Balancing Chemical Equations

29Net Ionic Equations

31 Six Types of Chemical Reactions

33 Voyage Through Equations

37Stoichiometry

41Yields

43 Boyle’s Law

45 Charles’ Law

47 Combined Gas Law

49 Ideal Gas Law

51 Gas Law Worksheet I

53 Gas Law Worksheet II

55 Molarity

59Concentration

60Acid/Base

62 pH

65Equilibrium

66Le Chatelier’s Principle

67Nuclear Chemistry

69 Organic Chemistry

70 Practice Final

Scientific Notation Worksheet

Convert the following numbers into scientific notation:

1)3,400 ______

2)0.000023 ______

3)101,000 ______

4)0.010 ______

5)45.01 ______

6)1,000,000 ______

7)0.00671 ______

8)4.50 ______

Convert the following numbers into standard notation:

9)2.30 x 104 ______

10)1.76 x 10-3 ______

11)1.901 x 10-7 ______

12)8.65 x 10-1 ______

13)9.11 x 103 ______

14)5.40 x 101 ______

15)1.76 x 100 ______

16)7.4 x 10-5 ______

Scientific Notation

Write each number in scientific notation.

0.07882 =

0.00000272338 =

118000 =

87200 =

0.00002786 =

0.000000664 =

450 =

74171.7 =

770 =

0.0000085 =

62360 =

147000 =

0.01388 =

0.0000445473 =

526 =

372123 =

583 =

0.0000573 =

0.000008738 =

0.000000813253 =

Write each number in standard format.

3.443 × 10-7 =

7.75763 × 10-7 =

5.8 × 10-7 =

1.525 × 106 =

6.58157 × 107 =

5.1821 × 10-4 =

1.21 × 10-7 =

5.2314 × 10-7 =

7.141 × 10-5 =

5.256 × 106 =

2.1463 x 102 =

2.86 x 10-3 =

7.62 x 10-2 =

6.443 x 107 =

7.284 x 10-4 =

3.0 x 10-5 =

1.88684 x 107 =

5.15 x 106 =

6.37 x 10-2 =

5.545 x 10-7 =

Write each number in standard format.

6.52 × 103 =

4.6322 × 104 =

8.66185 × 104 =

8.71 × 104 =

7.0 × 10-5 =

Write each number in scientific notation.

6520 =

46322 =

86618.5 =

87100 =

0.00007 =

Write each number in standard format.

5.513 x 107 =

4.12382 x 10-3 =

6.54766 x 10-5 =

5.3 x 103 =

8.32 x 10-2 =

Write each number in scientific notation.

55130000 =

0.00412382 =

0.0000654766 =

5300 =

0.0832 =

Significant Figures Practice Worksheet

How many significant figures do the following numbers have?

1)1234 _____

2)0.023 _____

3)890 _____

4)91010 _____

5)9010.0 _____

6)1090.0010 _____

7)0.00120 _____

8)3.4 x 104 _____

9)9.0 x 10-3 _____

10)9.010 x 10-2 _____

11)0.00030 _____

12)1020010 _____

13)780. _____

14)1000 _____

15)918.010 _____

16)0.0001 _____

17)0.00390 _____

18)8120 _____

19)7.991 x 10-10_____

20)72 _____

Significant Figures Worksheet

How many significant figures are in each of the following numbers?

1)5.40 ____6)1.2 x 103 ____

2)210 ____7)0.00120 ____

3)801.5 ____8)0.0102 ____

4)1,000 ____9)9.010 x 10-6____

5)101.0100 ____10)2,370.0 ____

Round these numbers to 3 significant digits.

11)1,566,311

12)2.7651 X 10 -3

13)84,592

14)0.0011672

15)0.07759

Give the number of significant digits in each of the following measurements:

1. 1278.50______7. 8.002______13. 43.050______

2. 120000______8. 823.012______14. 0.147______

3. 90027.00______9. 0.005789______15. 6271.91______

4. 0.0053567______10. 2.60______16. 6______

5. 670______11. 542000.______17. 3.47______

6. 0.00730______12. 2653008.0______18. 387465______

Round off the following numbers to three significant digits:

19. 120000______22. 4.53619______

20. 5.457______23. 43.659______

21. 0.0008769______24. 876493______

Density Problems

1) A block of aluminum occupies a volume of 15.0 mL and weighs 40.5 g. What is its density?

2) Mercury metal is poured into a graduated cylinder that holds exactly 22.5 mL. The mercury used to fill the cylinder weighs 306.0 g. From this information, calculate the density of mercury.

3) What is the weight of the ethyl alcohol that exactly fills a 200.0 mL container? The density of ethyl alcohol is 0.789 g/mL.

4) A rectangular block of copper metal weighs 1896 g. The dimensions of the block are 8.4 cm by 5.5 cm by 4.6 cm. From this data, what is the density of copper?

5) A flask that weighs 345.8 g is filled with 225 mL of carbon tetrachloride. The weight of the flask and carbon tetrachloride is found to be 703.55 g. From this information, calculate the density of carbon tetrachloride.

6) Calculate the density of sulfuric acid if 35.4 mL of the acid weighs 65.14 g.

7) Find the mass of 250.0 mL of benzene. The density of benzene is 0.8765 g/mL.

8) A block of lead has dimensions of 4.50 cm by 5.20 cm by 6.00 cm. The block weighs 1587 g. From this information, calculate the density of lead.

9) 28.5 g of iron shot is added to a graduated cylinder containing 45.50 mL of water. The water level rises to the 49.10 mL mark, From this information, calculate the density of iron.

10) What volume of silver metal will weigh exactly 2500.0 g. The density of silver is 10.5 g/cm3.

States of matter, elements, compounds, mixtures

1)List the three states of matter and describe their basic properties:

2) Classify the following as either elements, compounds, homogeneous mixtures (solutions) or heterogeneous mixtures:

a)copper (II) sulfate

b)Kool Aid

c)wood

d)plastic

e)lined paper

f)gadolinium

3)Why are homogeneous mixtures more difficult to separate than heterogeneous mixtures?

4)Why can’t elements be separated into smaller parts using chemical means?

Protons, Neutrons, and Electrons Practice Worksheet

Fill in the blanks in the following worksheet. Please keep in mind that the isotope represented by each space may NOT be the most common isotope or the one closest in atomic mass to the value on the periodic table.

Atomic
symbol / Atomic
number / Protons / Neutrons / Electrons / Atomic
mass
B / 6
11 / 24
31 / 37
39 / 89
29 / 35
43 / 100
Pb / 207
102 / 70
89 / 225
Mo / 53
81 / 206
100 / 159
No / 261
Yb / 172
106 / 159

The periodic table and oxidation states

Which group of the periodic table is most likely described by questions 1-5?

1)These elements are very strong oxidizers. ______

2)These elements have a charge of +2 when forming ionic compounds.

______

3)These elements are almost entirely unreactive. ______

4)These elements are radioactive. ______

5)These elements are all diatomic. ______

6)These elements are found in group 1 of the periodic table. ______

7)These elements are rare, have high densities, and are used for various industrial purposes.

______

For problems 8-11, describe the oxidation state of each element when it forms ionic compounds:

8)oxygen ______10)potassium ______

9)gallium ______11)nitrogen ______

For problems 12-15, determine the number of valence electrons each element has:

12)sulfur ______14)helium ______

13)carbon ______15)hydrogen ______

Electron Configuration Practice Worksheet

In the space below, write the unabbreviated electron configurations of the following elements:

1)sodium______

2)iron ______

3)bromine ______

4)barium ______

5)neptunium ______

In the space below, write the abbreviated electron configurations of the following elements:

6)cobalt______

7)silver______

8)tellurium______

9)radium______

10)lawrencium______

Determine what elements are denoted by the following electron configurations:

11)1s22s22p63s23p4 ______

12)1s22s22p63s23p64s23d104p65s1 ______

13)[Kr] 5s24d105p3 ______

14)[Xe] 6s24f145d6 ______

15)[Rn] 7s25f11 ______

Determine which of the following electron configurations are not valid:

16)1s22s22p63s23p64s24d104p5 ______

17)1s22s22p63s33d5 ______

18)[Ra] 7s25f8 ______

19)[Kr] 5s24d105p5 ______

20)[Xe] ______

Types of Solids Worksheet

Determine if the following compounds are metallic solids, ionic solids, network atomic solids, molecular solids, or amorphous solids based on their properties. These are all actual chemical compounds.

1)This material forms crumbly crystals and has a melting point of 16.60 Celsius. It has a low density in solid form.

______(acetic acid)

2)This material forms very hard colorless crystals. It does not dissolve in water and burns at high temperatures.

______(diamond)

3)This material forms colorless crystals that have a melting point of 6610 C. It is hard, brittle, and dissolves well in water.

______(sodium iodide)

4)This material forms silver crystals that do not dissolve in water and have a melting point of 14140 C. This material is very hard and is not a good conductor of electricity.

______(silicon)

5)This material is hard and melts at a temperature of 16100C. It dissolves only with difficulty in very reactive acids and doesn’t conduct electricity when molten. It forms colorless crystals.

______(quartz)

6)This material is soft and doesn’t form crystals. It has a melting point of 6600 C. It doesn’t dissolve in water. It is used as a structural material in the construction of airplanes and rockets.

______(aluminum)

7)This material is easily scratched. It is black and has a melting point of 1850 C. It is used for applications where lightweight, nonstructural materials are required.

______(plastic)

Naming Ionic Compounds

NameMolar Mass

1)Na2CO3______

2)NaOH ______

3)MgBr2 ______

4)KCl ______

5)FeCl2 ______

6)FeCl3 ______

7)Zn(OH)2 ______

8)Be2SO4 ______

9)CrF2 ______

10)Al2S3 ______

11)PbO ______

12)Li3PO4 ______

13)TiI4 ______

14)Co3N2 ______

15)Mg3P2 ______

16)Ga(NO2)3 ______

17)Ag2SO3 ______

18)NH4OH ______

19)Al(CN)3 ______

20)Be(CH3COO)2 ______
For the following compounds, give the formulas and the molar masses:

FormulaMolar Mass

22)sodium phosphide ______

23)magnesium nitrate ______

24)lead (II) sulfite ______

25)calcium phosphate ______

26)ammonium sulfate ______

27)silver cyanide ______

28)aluminum sulfide ______

29)beryllium chloride ______

30)copper (I) arsenide ______

31)iron (III) oxide ______

32)gallium nitride ______

33)iron (II) bromide ______

34)vanadium (V) phosphate ______

35)calcium oxide ______

36)magnesium acetate ______

37)aluminum sulfate ______

38)copper (I) carbonate ______

39)barium oxide ______

40)ammonium sulfite ______

41)silver bromide ______

42)lead (IV) nitrite ______

Naming Covalent Compounds Worksheet

Write the formulas for the following covalent compounds:

1)antimony tribromide ______

2)hexaboron silicide ______

3)chlorine dioxide ______

4)hydrogen iodide ______

5)iodine pentafluoride ______

6)dinitrogen trioxide ______

7)ammonia ______

8)phosphorus triiodide ______

Write the names for the following covalent compounds:

9)P4S5 ______

10)O2 ______

11)SeF6 ______

12)Si2Br6 ______

13)SCl4 ______

14)CH4 ______

15)B2Si ______

16)NF3 ______

Compound Naming and Formula Writing

1)copper (II) acetate ______

2)sodium hydroxide ______

3)lithium oxide ______

4)cobalt (III) carbonate ______

5)aluminum sulfide ______

6)ammonium cyanide ______

7)iron (III) phosphide ______

8)vanadium (V) phosphate ______

9)sodium permanganate ______

10)manganese (III) fluoride ______

11)beryllium nitrate ______

12)nickel (III) sulfite ______

13)potassium oxide ______

14)silver bromide ______

15)zinc phosphate ______

16)copper (II) bicarbonate ______

17)nickel (II) selenide ______

18)manganese (IV) carbonate ______

19)lead (IV) nitride ______

20)tin (II) hydroxide ______

21)lithium arsenide ______

22)chromium (VI) sulfate ______

23)calcium bromide ______

24)ammonium sulfate ______

25)copper (II) oxide ______

26)platinum (IV) phosphate ______

27)aluminum carbonate ______

28)silver nitrate ______

29)magnesium acetate ______

30)nickel (III) cyanide ______

31)vanadium (IV) phosphate ______

32)silver sulfate ______

33)cobalt (III) sulfide ______

34)iron (II) sulfite ______

35)copper (II) nitrite ______

36)nickel (II) hydroxide ______

37)zinc nitride ______

38)manganese (VII) nitrate ______

39)gallium sulfate ______

40)sodium nitrate ______

Finding Heats of Reaction from Heats of Formation

1)Calcium carbonate decomposes at high temperature to form carbon dioxide and calcium oxide:

CaCO3 CO2 + CaO

Given that the heat of formation of calcium carbonate is –1207 kJ/mol, the heat of formation of carbon dioxide is –394 kJ/mol, and the heat of formation of calcium oxide is –635 kJ/mol, determine the heat of reaction.

2)Carbon tetrachloride can be formed by reacting chlorine with methane:

CH4 + 2 Cl2 CCl4 + 2 H2

Given that the heat of formation of methane is –75 kJ/mol and the heat of formation of carbon tetrachloride is –135 kJ/mol, determine the heat of reaction.

3)When potassium chloride reacts with oxygen under the right conditions, potassium chlorate is formed:

2 KCl + 3 O2 2KClO3

Given that the heat of formation of potassium chloride is –436 kJ/mol and the heat of formation of potassium chlorate is –391 kJ/mol, determine the heat of reaction.

Calorimetry Practice Worksheet

1)Compound A is burned in a bomb calorimeter that contains 2.50 liters of water. If the combustion of 0.175 moles of this compound causes the temperature of the water to rise 45.00 C, what is the molar heat of combustion of compound A? The heat capacity of water is 4.184 J / g0C.

2)Compound B is burned in a bomb calorimeter that contains 1.50 liters of water. When I burned 50.0 grams of compound B in the calorimeter, the temperature rise of the water in the calorimeter was 35.00 C. If the heat of combustion of compound B is 2,150 kJ/mol, what is the molar mass of compound B?

3)The molar heat of combustion of compound C is 1,250 kJ/mol. If I were to burn 0.115 moles of this compound in a bomb calorimeter with a reservoir that holds 2.50 L of water, what would the expected temperature increase be?

Lewis Structures, VSEPR, Polarity, IM Forces

For each of the following molecules, draw the Lewis structure (with any resonance structures, if applicable), indicate the molecular shapes and bond angles, indicate the molecular polarity (if any), and identify the major intermolecular force in each compound. Hint – in this worksheet, as in all chemistry problems you’ll see, polyatomic ions aren’t drawn as big lines of atoms.

1)carbon tetrafluoride

2)BF3

3)NF3

4)H2CS

5)carbonate ion

6)CH2F2

7)nitrate ion

8)O2

9)PF3

10)H2S

More Fun With Lewis Structures

For each of the following compounds or ions, draw the Lewis structures (with resonance structures, if applicable), show the bond angles and molecular shapes, and indicate whether the molecule or ion is polar.

1)PS3-1

2)SHF

3)CF2S

4)BH3

5)SF2

6)P2H4

Word Equations

Write the word equations below as chemical equations and balance:

1)Zinc and lead (II) nitrate react to form zinc nitrate and lead.

______

2)Aluminum bromide and chlorine gas react to form aluminum chloride and bromine gas.

______

3)Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride.

______

4)Potassium metal and chlorine gas combine to form potassium chloride.

______

5)Aluminum and hydrochloric acid react to form aluminum chloride and hydrogen gas.

______

6)Calcium hydroxide and phosphoric acid react to form calcium phosphate and water.

______

7)Copper and sulfuric acid react to form copper (II) sulfate and water and sulfur dioxide.

______

8)Hydrogen gas and nitrogen monoxide react to form water and nitrogen gas.

Writing Complete Equations Practice

For each of the following problems, write complete chemical equations to describe the chemical process taking place. Important note: There are a few physical processes on this sheet – remember, you can’t write an equation for a physical process!

1)When lithium hydroxide pellets are added to a solution of sulfuric acid, lithium sulfate and water are formed.

2)When dirty water is boiled for purification purposes, the temperature is brought up to 1000 C for 15 minutes.

3)If a copper coil is placed into a solution of silver nitrate, silver crystals form on the surface of the copper. Additionally, highly soluble copper (I) nitrate is generated.

4)When crystalline C6H12O6 is burned in oxygen, carbon dioxide and water vapor are formed.

5)When a chunk of palladium metal is ground into a very fine powder and heated to drive off any atmospheric moisture, the resulting powder is an excellent catalyst for chemical reactions.

Balancing Chemical Equations

Balance the equations below:

1)____ N2 + ____ H2 ____ NH3

2)____ KClO3 ____ KCl + ____ O2

3)____ NaCl + ____ F2 ____ NaF + ____ Cl2

4)____ H2 + ____ O2 ____ H2O

5)____ Pb(OH)2 + ____ HCl  ____ H2O + ____ PbCl2

6)____ AlBr3 + ____ K2SO4 ____ KBr + ____ Al2(SO4)3

7)____ CH4 + ____ O2 ____ CO2 + ____ H2O

8)____ C3H8 + ____ O2 ____ CO2 + ____ H2O

9)____ C8H18 + ____ O2 ____ CO2 + ____ H2O

10)____ FeCl3 + ____ NaOH  ____ Fe(OH)3 + ____NaCl

11)____ P + ____O2 ____P2O5

12)____ Na + ____ H2O  ____ NaOH + ____H2

13)____ Ag2O  ____ Ag + ____O2

14)____ S8 + ____O2 ____ SO3

15)____ CO2 + ____ H2O  ____ C6H12O6 + ____O2

16)____ K + ____ MgBr  ____ KBr + ____ Mg

17)____ HCl + ____ CaCO3 ____ CaCl2 + ____H2O + ____ CO2

18)____ HNO3 + ____ NaHCO3 ____ NaNO3 + ____ H2O + ____ CO2

19)____ H2O + ____ O2 ____ H2O2

20)____ NaBr + ____ CaF2 ____ NaF + ____ CaBr2

21)____ H2SO4 + ____ NaNO2 ____ HNO2 + ____ Na2SO4

Net Ionic Equations

I. Short Answer:

1. What is an ionic equation? ______

2. What is a spectator ion? ______

3. What is a net ionic equation? ______

II. For each of the following, first balance the equation. Then write out (cie) the complete ionic equation and (nie) the net ionic equation

for each.

4) ___AgNO3(aq) + ___ CaCl2(aq) ----> ___ AgCl(s) + ___ Ca(NO3)2(aq)

cie) ______

nie) ______

5) ___ Cu(s) + ___AgNO3(aq) ----> ___Ag(s) + ___ Cu(NO3)2(aq)

cie) ______

nie) ______

6) ___ HCl(aq) + ___ Zn(s) ----> ___ H2(g) + ___ ZnCl2(aq)

cie) ______

nie) ______

Practicing Net Ionic Equations

Directions: Provide (a) the balanced equation and (b) write out the net ionic equation for each

of the following. Make sure your balanced equation has the right (aq)’s, (s)’s, (l)’s and (g)’s.

1. (a) ____ Na2CO3 (___) + ___ Ca(OH)2(___) ---> ___ NaOH (___) + ___ CaCO3 (___)

(b)______

2. Solid zinc in aqueous hydrogen chloride produces hydrogen gas and aqueous zinc chloride.

(a)______

(b)______

3. Silver nitrate + sodium chloride

(a)______

(b)______

4. (a)____ KBr (aq) + ___ Cl2(g) ---> ___ KCl (aq) + ___ Br2 (l)

(b)______

5. Aqueous aluminum sulfate plus aqueous ammonium chromate reacts to form aqueous

ammonium sulfate plus solid aluminum chromate.

(a)______

(b)______

6. (a)____ Mg(HCO3)2 (aq) + ___ HCl(aq) ---> ___ MgCl2(aq) + ___ H2O (l)+ ___ CO2 (g)

(b)______

7. calcium chloride plus lithium hydroxide

(a)______

(b)______

8. (a)____ KI (___) + ___ Pb(NO3)2(___) ---> ___ PbI2 (___) + ___ KNO3 (___)

(b)______

9. Solid aluminum metal in aqueous hydrogen sulfate produces hydrogen gas and aqueous

aluminum sulfate.

(a)______

(b)______

Six Types of Chemical Reaction Worksheet

Balance the following reactions and indicate which of the six types of chemical reaction are being represented:

1)____ NaBr + ____ Ca(OH)2 ___ CaBr2 + ____ NaOH

Type of reaction: ______

2)____ NH3+ ____ H2SO4 ____ (NH4)2SO4

Type of reaction: ______

3)____ C5H9O + ____ O2 ____ CO2 + ____ H2O

Type of reaction: ______

4)____ Pb + ____ H3PO4 ____ H2 + ____ Pb3(PO4)2

Type of reaction: ______

5)____ Li3N + ____ NH4NO3 ___ LiNO3 + ___ (NH4)3N

Type of reaction: ______

6)____ HBr + ___ Al(OH)3 ___ H2O + ___ AlBr3

Type of reaction: ______

7)What’s the main difference between a double displacement reaction and an acid-base reaction?

8)Combustion reactions always result in the formation of water. What other types of chemical reaction may result in the formation of water? Write examples of these reactions on the opposite side of this paper.

Predicting Reaction Products

Balance the equations and predict the products for the following reactions:

1)____ Na + ____ FeBr3

2)____ NaOH + ____ H2SO4

3)____ C2H4O2 + ____ O2

4)____ NH3 + ____ H2O 

5)____ PbSO4 + ____ AgNO3

6)____ PBr3

7)____ HBr + ____ Fe 

8)____ KMnO4 + ____ ZnCl2

9)____MnO2 + ____ Sn(OH)4

10)____ O2 + ____ C5H12O2

11)____ H2O2

12)____ PtCl4 + ____ Cl2

A Voyage through Equations

After working on this worksheet, you should be able to do the following:

1)Given an equation, you should be able to tell what kind of reaction it is.

2)Predict the products of a reaction when given the reactants.

Section 1: Identify the type of reaction

For the following reactions, indicate whether the following are examples of synthesis, decomposition, combustion, single displacement, double displacement, or acid-base reactions:

1)Na3PO4 + 3 KOH  3 NaOH + K3PO4 ______

2)MgCl2 + Li2CO3 MgCO3 + 2 LiCl ______

3)C6H12 + 9 O2 6 CO2 + 6 H2O ______

4)Pb + FeSO4 PbSO4 + Fe ______

5)CaCO3 CaO + CO2 ______

6)P4 + 3 O2 2 P2O3 ______

7)2 RbNO3 + BeF2 Be(NO3)2 + 2 RbF ______

8)2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag ______

9)C3H6O + 4 O2 3 CO2 + 3 H2O ______

10)2 C5H5 + Fe  Fe(C5H5)2 ______

11)SeCl6 + O2 SeO2 + 3Cl2 ______

12)2 MgI2 + Mn(SO3)2 2 MgSO3 + MnI4 ______

13)O3  O. + O2 ______

14)2 NO2 2 O2 + N2______

Section 2: Practicing equation balancing

Before you can write a balanced equation for a problem which asks you to predict the products of a reaction, you need to know how to balance an equation. Because some of you may not fully remember how to balance an equation, here are some practice problems:

1)__ C6H6 + __ O2 __ H2O + __ CO2

2)__ NaI + __ Pb(SO4)2 __ PbI4 + __ Na2SO4

3)__ NH3 + __ O2__ NO + __ H2O

4)__ Fe(OH)3 __ Fe2O3 + __ H2O

5)__ HNO3 + __ Mg(OH)2 __H2O + __ Mg(NO3)2

6)__ H3PO4 + __ NaBr  __ HBr + __ Na3PO4

7)__ C + __ H2 __ C3H8

8)__ CaO + __ MnI4 __ MnO2 + __ CaI2

9)__ Fe2O3 + __ H2O  __ Fe(OH)3

10)__ C2H2 + __ H2 __ C2H6

11)__ VF5 + __ HI  __ V2I10 + __ HF

12)__ OsO4 + __ PtCl4 __ PtO2 + __ OsCl8

13)__ CF4 + __ Br2 __ CBr4 + __ F2

14)__ Hg2I2 + __ O2 __ Hg2O + __ I2

15)__ Y(NO3)2 + __ GaPO4 __ YPO4 + __ Ga(NO3)2

Section 3: Predicting the products of chemical reactions

Predict the products of the following reactions:

1)__ Ag + __CuSO4

Type:______

2)__ NaI + __ CaCl2

Type:______

3)__ O2 + __ H2

Type:______

4)__ HNO3 + __ Mn(OH)2

Type:______

5)__ AgNO2 + __ BaSO4

Type:______

6)__ HCN + __ CuSO4

Type:______

7)__ H2O + __ AgI 

Type:______

8)__ HNO3 + __Fe(OH)3

Type:______

9)__ LiBr + __ Co(SO3)2

Type:______

10)__ LiNO3 + __Ag 

Type:______

11)__ N2 + __ O2

Type:______

12)__ H2CO3

Type:______

13)__ AlCl3 + __ Cs 

Type:______

14)__ Al(NO3)3 + __ Ga 

Type:______

15)__ H2SO4 + __ NH4OH 

Type:______

16)__ CH3COOH + __ O2

Type:______

17)__ C4H8 + __ O2

Type:______

18)__ KCl + __ Mg(OH)2

Type:______

19)__ Zn + __ Au(NO2)2

Type:______

20)__ KOH + __ H2SO4

Type:______

21)__ BaS + __ PtCl2

Type:______

22)__ Na2O 

Type:______

Stoichiometry

How many moles of O2 should be supplied to

burn 1 mol of C3H8 (propane) molecules in a camping stove?

How many moles of O2 molecules should be

supplied to burn 1 mol of CH4 molecules in a domestic furnace?

Sodium thiosulfate (Na2S2O3), photographer’s

“hypo” reacts with unexposed silver bromide in the film emulsion to form sodium bromide and a compound of formula Na5[Ag(S2O3) 3]. How many moles of Na2S2O3 formula units are needed to make 0.10 mol of AgBr soluble?

Calculate the mass of alumina (Al2O3)

produced when 100 g of aluminum burns in oxygen.

“Slaked lime,” Ca(OH) 2, is formed from

“quick-lime” (CaO) by adding water. What mass of water is needed to convert 10 kg of quicklime to slaked lime? What mass of slaked lime is produced?

Camels store the fat tristearin (C57H110O6) in

the hump. As well as being a source of energy, the fat is a source of water, because when it is used the reaction

2 C57H110O6(s) + 163 O2(g) 

114 CO2(g) + 110 H2O(l)

takes place. What mass of water is available from 1.0 kg of fat?

The compound diborane (B2H6) was at one

time considered for use as a rocket fuel. How many grams of liquid oxygen would a rocket have to carry to burn 10 kg of diborane completely? (The products of the combustion are B2O3 and H2O.)

Given the balanced chemical equation

Br2 + 2 NaI  2 NaBr + I2

How many moles of sodium bromide (NaBr) could be produced from 0.172 mol of bromine (Br2)?

How many formula units of calcium oxide

(CaO) can be produced from 4.9 x 105 molecules of oxygen gas (O2) that react with calcium (Ca) according to this balanced chemical equation?

2 Ca(s) + O2 (g)  2 CaO(s)

Aluminum metal (Al) reacts with sulfur (S) to

produce aluminum sulfide (Al2S3) according to this balanced chemical equation:

2 Al(s) + 3 S(s)  Al2S3(s)

How many atoms of aluminum will react completely with 1.33 x 1024 atoms of sulfur?

Limiting Reagents

What is the maximum mass of methane (CH4)

that can be burned if only 1.0 g of oxygen is available?

What is the maximum mass of glucose

(C6H12O6) that can be burned in 10 g of oxygen?

13. The solid fuel in the booster stage of the space shuttle is a mixture of ammonium perchlorate

and aluminum powder, which react as follows:

6 NH4ClO4(s) + 10 Al(s)  5 Al2O3(s) +

3 N2(g) + 6 HCl(g) + 9 H2O(g)

What mass of aluminum should be mixed with 5.0

x 103 kg of ammonium perchlorate, if the reaction

proceeds as stated?

14. A solution containing 5.0 g of silver nitrate was mixed with another containing 5.0 g of potassium

chloride. Which was the limiting reagent for the

precipitation of silver chloride?

Given the balanced chemical equation

2 Ag + I2  2 AgI

How many atoms of silver metal (Ag) are required to react completely with 531.8 g of iodine (I2) to produce silver iodide (AgI)?

16. The theoretical yield of ammonia in an industrial synthesis was 550 tons, but only 480 tons was

obtained. What was the percentage yield of the

reaction?

Calculate the volume occupied by 16.3 moles of

nitrogen gas (N2) at STP.

How many moles of fluorine gas (F2) are

contained in 0.269 dm3 container at STP?

Assuming that the gases are all at STP, find the

volume of nitrogen dioxide gas (NO2) that could be produced from 71.11 dm3 of nitrogen gas (N2) according to this balanced chemical equation.

N2(g) + 2 O2(g)  2 NO2(g)

How many moles of oxygen (O2) would be

needed to produce 79.60 moles of sulfur trioxide (SO3) according to the following balanced chemical equation?

2 SO2 + O2  2 SO3

21. How many grams of water will be produced from 50 g hydrogen reacting with 50 g oxygen?

Think Critically

22. The reaction of 1 mol of C to form carbon monoxide in the reaction 2 C(s) + O2(g)  2 CO(g) releases 113 kJ of heat. How much heat will be released by the combustion of 100 g of C according the the above information?

According to the balanced chemical equation;

how many atoms of silver will be produced from combining 100 g of copper with 200 g of silver nitrate?

Cu(s) + 2 AgNO3(aq)  Cu(NO3) 2(aq) + 2 Ag(s)

According to the balanced chemical equation;

how many moles of SO2(g) will be produced when 1.5 x 108 molecules of zinc sulfide react with 1000 dm3 of oxygen gas? Assume a 75% yield.

2 ZnS(s) + 3 O2 (g)  2 ZnO(s) + 2 SO2(g)