Unit IV

Chemistry 11

Reactions

Lesson Day     Date                Assignment

1.             1                     Synthesis and Decomposition Reactions

2.             2                      Single Replacement Reactions

3.             Lab Report      Single Replacement Reactions Lab

4.             3                      Double Replacement Reactions

5.             Lab Report      Double Replacement Reactions Lab

6.             4                      CombustionReview

7.             5                      Formula and Ionic Equations

8.             6                      Lab Report      Reactions Lab Day 1

9.             6                      Lab Report      Reactions Lab Day 2       Reactions Practice Test 1

10.             7                      Reactions PracticeTest 2

11.                               8                      Reactions Practice Test 3

12.                                                       Test

Worksheet #1 Synthesis and Decomposition Reactions

Predict and balance the following synthesis and decomposition reactions. Assume that all reactions will occur. Use abbreviations to indicate the phase of reactants and products: (aq) (s) (l) (g).

1. A sample of mercury II oxide is heated.

2HgO_(s) → 2Hg_(l) + O_2(g)

2. Sulfur dioxide SO₂ gas is heated.

8SO_2(g) → S_8(s) + 8O_2(g)

3. Aluminum is reacted with iodine.

2Al_(s) + 3I_2(s) → 2AlI_3(s)

 4. Liquid hydrogen peroxide composes to water and another common gas..

2H₂O_2(l) → 2H₂O_(l) + O_2(g)

5. Solid lithium reacts with sulphur.

16Li_(s) + S_8(s) → 8Li₂S_(s)

 6. Molten aluminum chloride is electrolyzed.

2AlCl_3(l) → 2Al_(s) + 3Cl_2(g)

7. Sodium is added to a container of iodine vapor.

2Na_(s) + I_2(g) → 2NaI_(s)

8. Molten calcium chloride is electrolyzed.

CaCl_2(l) → Ca_(s) + Cl_2(g)

9.         Ibuprofen has a chemical formula of C13H18O2.  A very small sample of ibuprofen has 85 atoms of carbon.  How many atoms of hydrogen does this sample contain?

85 at C     x     1 molecule     x     18 at H           =      1.2 x 10² at H   or    120 at      2 sig figs!
13 at C                  1 molecule

10.  A volume of a gas called methyl mercaptan,  a chemical that makes human flatulence smell bad, weighs 0.5963 g.  An equal volume of H2 weighs 0.02477 g.  Calculate the molecular mass of the gas.  Assuming that this gas is an element, what is the chemical formula of the gas? Hint: Google is your friend.

 Gas x      =     0.5963        x       2.02 g/mol          =      48.6      2 sig figs!       CH₄S
H₂                  0.02477

11.  Psilocybin is a psychedelic chemical found in magic mushrooms and is 50.40 % C, 6.545 % H, 9.450 % N, 22.40 % O and 10.85 % P. Determine the empirical formula for psilocybin.

C₂₄H₃₇N₄O₈P₂

Worksheet #2 Single Replacement Reactions

Using the activity series, predict and balance the following single replacement reactions. Use abbreviations to indicate the appropriate phase of reactants and products. For those that do not react, write no reaction.

1. A piece of copper is dropped into a container of water.

Cu_(s) + HOH_(l) → No Reaction. H is more active than Cu.

2. Liquid bromine is added to a container of sodium iodide crystals.

Br_2(l) + 2NaI_(s) → I_2(s) + 2NaBr_(s)

3. An aluminum strip is immersed in a solution of silver nitrate.

Al_(s) + 3AgNO_3(aq) → 3Ag_(s) + Al(NO₃)_3(aq)

4. Zinc pellets are added to a sulfuric acid solution.

Zn_(s) + H₂SO_4(aq) → H_2(g) + ZnSO_4(aq)

5. Fluorine gas is bubbled into a solution of aluminum chloride.

3F_2(g) + 2AlCl_3(aq) → 3Cl_2(g) + 2AlF_3(aq)

6. Magnesium turnings are added to a solution of lead (II) acetate.

Mg_(s) + Pb(CH₃COO)_2(aq) → Pb_(s) + Mg(CH₃COO)_2(aq)

7. Iodine crystals are added to a solution of sodium chloride.

I_2(s) + NaCl_(aq) → No Reaction. Cl₂ is more active than I₂.

8. Calcium metal is added to a solution of nitric acid.

Ca_(s) + 2HNO_3(aq) → H_2(g) + Ca(NO₃)_2(aq)

9. A pea-sized piece of lithium is added to water.

2Li_(s) + 2HOH_(l) → H_2(g) + 2LiOH_(aq)

10. A solution of iron (III) chloride is poured over a piece of platinum wire.

Pt_(s) + FeCl_3(aq) → No Reaction. Fe is more active than Pt.

11.        Monosodium glutamate (MSG), a food-flavor enhancer, has been blamed for   “Chinese restaurant syndrome,” the symptoms of which are headaches and chest pains. MSG has the following composition by mass: 35.51 % C, 4.77 % H, 37.85 % O, 8.29 % N, and 13.60 % Na.

NaC₅H₈NO₄

13.     Chocolate contains phenylethylamine - the same chemical that is released in your brain when you fall in love. It is also believed that phenylethylamine in turn causes the brain to release mesolimbic dopamine in the pleasure centers of the brain, another chemical that is produced during more intimate love. If the formula for this compound is C₈H₁₁N, calculate its percentage composition to 3 sig figs.

79.3 % C

9.17 % H

11.6 % N

Worksheet #3 Double Replacement Reactions

Predict and balance the following Double Replacement reactions. Include all phase symbols. Use your solubility table to predict.

1. Silver nitrate + Potassium sulphate

2AgNO_3(aq) + K₂SO_4(aq) → Ag₂SO_4(s) + 2KNO_3(aq)

2. Ammonium chloride + Cobalt (II) sulfate

NH₄Cl_(aq) + CoSO_4(aq) → No Reaction as both possible products are high solubility.

3. Lead II nitrate + Sodium chloride

Pb(NO₃)_2(aq) + 2NaCl_(aq) → PbCl_2(s) + 2NaNO_3(aq)

4. Zinc bromide + Cesium hydroxide

ZnBr_2(aq) + 2CsOH_(aq) → Zn(OH)_2(s) + 2CsBr_(aq)

5. Ammonium sulfide + Lead II nitrate

(NH₄)₂S_(aq) + Pb(NO₃)_2(aq) → PbS_(s) + 2NH₄NO_3(aq)

6. Iron III sulfate + Barium iodide

Fe₂(SO₄)_3(aq) + 3BaI_2(aq) → 3BaSO_4(s) + 2FeI_3(aq)

7. Chromium III bromide + Sodium nitrate

CrBr_3(aq) + NaNO_3(aq) → No Reaction, both products are soluble.

8. Rubidium phosphate + Titanium IV nitrate

4Rb₃PO_4(aq) + 3Ti(NO₃)_4(aq) → Ti₃(PO₄)_4(s) + 12RbNO_3(aq)

9. Ammonium carbonate + Nickel II chloride

(NH₄)₂CO_3(aq) + NiCl_2(aq) → NiCO_3(s) + 2NH₄Cl

10. Tin IV nitrate + Potassium sulfite

Sn(NO₃)_4(aq) + 2K₂SO_3(aq) → Sn(SO₃)_2(s) + 4KNO_3(aq)

11. Ammonium sulfate and Potassium hydroxide

No Reaction as both possible products has high solubility.

12. Cobalt II chloride is combined with Silver nitrate

CoCl_2(aq) + 2AgNO_3(aq) → 2AgCl_(s) + Co(NO₃)_2(aq)

Complete the following combustion reactions. Include all phase symbols.

13. 2C₄H_10(g) + 13O_2(g) → 8CO_2(g) + 10H₂O_(l)

14. C₆H_12(l) + 9O_2(g) → 6CO_2(g) + 6H₂O_(l)

15. C₂₂H_42(l) + 32.5O_2(g) → 22CO_2(g) + 21H₂O_(l)

16. C₆H₁₂O_6(s) + 6O_2(g) → 6CO_2(g) + 6H₂O_(l)

17. 2C₁₂H₂₄O_11(s) + 25O_2(g) → 24CO_2(g) + 24H₂O_(l)

Complete the following acid carbonate reactions. Include all phase symbols.

18. 2HCl_(aq) + CaCO_3(s) → CO_2(g) + CaCl_2aq) + H₂0_(l)

19. H₂SO_4(aq) + BaCO_3(s) → CO_2(g) + BaSO_4(s) + H₂0_(l)

20. 2H₃PO_4(aq) + 3Na₂CO_3(s) → 3CO_2(g) + 2Na₃PO_4(s) + 3H₂0_(l)

Worksheet 4 Reactions

1. Zinc is reacted with phosphorus.

6Zn_(s) + P_4(s) → 2Zn₃P_2(s)

2. A solution of cobalt (II) nitrate is reacted with a solution of sodium carbonate.

Co(NO₃)_2(aq) + Na₂CO_3(aq) → CoCO_3(s) + 2NaNO_3(aq)

3. Magnesium metal is placed in a solution of zinc chloride.

Mg_(s) + ZnCl_2(aq) → Zn_(s) + MgCl_2(aq)

4. Iron (III) oxide is decomposed.

2Fe₂O_3(s) → 4Fe_(s) + 3O_2(g)

5. Octane, C₈H₁₈, is burned as a fuel in cars.

2C₈H_18(l) + 25O_2(g) → 16CO_2(g) + 18H₂O_(l)

6. Lithium reacts with water.

2Li_(s) + 2H₂O_(l) → H_2(g) + 2LiOH_(aq)

7. Sodium hydroxide solution is reacted with sulphuric acid.

2NaOH_(aq) + H₂SO_4(aq) → Na₂SO_4(aq) + 2H₂O_(l)

Note that acid base reactions do not require a low solubility product!

8. Phosphoric acid reacts with barium hydroxide.

2H₃PO_4(aq) + 3Ba(OH)_2(s) → Ba₃(PO₄)_2(s) + 6HOH_(l)

9. Hydrochloric acid reacts with barium carbonate.

2HCl_(aq) + BaCO_3(s) → CO_2(g) + BaCl_2(aq) + H₂O_(l) Remember this one from the lab!

10. The decomposition of sodium sulphide using electrolysis.

8Na₂S_(s) → 16Na_(s) + S_8(s)

11. Calcium reacts with water.

Ca_(s) + 2HOH_(l) → H_2(g) + Ca(OH)_2(s)

12. Barium reacts with phosphoric acid.

3Ba_(s) + 2H₃PO_4(aq) → 3H_2(g) + Ba₃(PO₄)_2(s)

13. Barium nitrate and Aluminum sulphate react in solution.

3Ba(NO₃)_2(aq) + Al₂(SO₄)_3(aq) → 3BaSO_4(s) + 2Al(NO₃)_3(aq)

Worksheet 5 Formula and Ionic Equations

Write dissociation Equations for the following.

1. Na₃PO_4(s) → 3Na⁺_(aq) + PO₄^-3_(aq)

2. Mg(OH)_2(s) → Mg⁺²_(aq) + 2 OH^-_(aq)

3. (NH₄)₂Cr₂O_7(s) → 2NH₄ ⁺_(aq) + Cr₂O₇^-2_(aq)

4. H₃PO_4(s) → 3H⁺_(aq) + PO₄^-3_(aq)

5. CaC₂O_4(s) → Ca⁺²_(aq) + C₂O₄^-2_(aq)

6. Ga(SCN)_3(s) → Ga⁺³_(aq) + 3SCN^-_(aq)

7. Ba(HCO₃)_2(s) → Ba⁺²_(aq) + 2HCO₃^-_(aq)

8. (NH₄)₂SO_4(s) → 2NH₄ ⁺_(aq) + SO₄^-2_(aq)

9. Al₂(CO₃)_3(s) → 2Al⁺³_(aq) + 3CO₃^-2_(aq)

10. Sr(ClO)_2(s) → Sr⁺²_(aq) + 2ClO^-_(aq)

Complete the formula equation, complete ionic equation, and net ionic equation:

1. 2AgNO_3(aq) + Na₂SO_4(aq) → Ag₂SO_4(s) + 2NaNO_3(aq)

2Ag⁺_(aq) + 2NO₃^-_(aq) + 2Na⁺_(aq) + SO₄^2-_(aq) → Ag₂SO_4(s) + 2Na⁺_(aq) + 2NO₃^-_(aq)

2Ag⁺_(aq) + SO₄^2-_(aq) → Ag₂SO_4(s)

2. 2H₃PO_4(aq) + 3Sr(OH)_2(aq) → Sr₃(PO₄)_2(s) + 6HOH_(l)

6H⁺_(aq) + 2PO₄^3-_(aq) + 3Sr²⁺ + 6OH^-_(aq) → Sr₃(PO₄)_2(s) + 6HOH_(l)

6H⁺_(aq) + 2PO₄^3-_(aq) + 3Sr²⁺ + 6OH^-_(aq) → Sr₃(PO₄)_2(s) + 6HOH_(l)

3. 2Fe(NO₃)_3(aq) + 3Zn_(s) → 2Fe_(s) + 3Zn(NO₃)_2(aq)

2Fe³⁺_(aq) + 6NO₃^-_(aq) + 3Zn_(s) → 2Fe_(s) + 3Zn²⁺_(aq) + 6NO₃^-_(aq)

2Fe³⁺_(aq) + 3Zn_(s) → 2Fe_(s) + 3Zn²⁺_(aq)

4. H₂SO_4(aq) + 2NaOH_(aq) → Na₂SO_4(aq) + 2HOH_(l)

2H⁺_(aq) + SO₄^2-_(aq) + 2Na⁺_(aq) + 2OH^-_(aq) → 2Na⁺_(aq) + SO₄^2-_(aq) + 2HOH_(l)

H⁺_(aq) + OH^-_(aq) → HOH_(l)

5. H₃PO_4(aq) + 3KOH_(aq) → K₃PO_4(aq) + 3HOH_(l)

3H⁺_(aq) + PO₄^3-_(aq) + 3K⁺_(aq) + 3OH^-_(aq) → 3K⁺     + PO₄^3-_(aq) + 3HOH_(l)

H⁺_(aq) + OH^-_(aq) → HOH_(l)

6. 3Ca(NO₃)_2(aq) + 2Na₃PO_4(aq) → Ca₃(PO₄)_2(s) + 6NaNO_3(aq)

3Ca²⁺_(aq) + 6NO₃^-_(aq) + 6Na⁺_(aq) + 2PO₄^3-_(aq) → Ca₃(PO₄)_2(s) + 6Na⁺_(aq) + 6NO₃^-_(aq)

3Ca²⁺_(aq) + 2PO₄^3-_(aq) → Ca₃(PO₄)_2(s)

7. Zn(s) + 2HCl_(aq) → H_2(g) + ZnCl_2(aq)

Zn(s) + 2H⁺_(aq) + 2Cl^-_(aq) → H_2(g) + Zn²⁺_(aq) + 2Cl^-_(aq)

Zn(s) + 2H⁺_(aq) → H_2(g) + Zn²⁺_(aq)

8. Sr(OH)_{2 (aq)} + ZnSO_{4 (aq)} → Zn(OH)_{2 (s)} + SrSO_{4 (s)}

Sr²⁺_(aq) + 2OH^-_(aq) + Zn²⁺_(aq) + SO₄^2-_(aq) → Zn(OH)_{2 (s)} + SrSO_{4 (s)}

Sr²⁺_(aq) + 2OH^-_(aq) + Zn²⁺_(aq) + SO₄^2-_(aq) → Zn(OH)_{2 (s)} + SrSO_{4 (s)}

9. Ca_(s) + 2HOH_(l) → H_2(g) + Ca(OH)_2(s)

Ca_(s) + 2HOH_(l) → H_2(g) + Ca(OH)_2(s)

Ca_(s) + 2HOH_(l) → H_2(g) + Ca(OH)_2(s)

Note: only aqueous ionic compounds are broken into ions.

10. AlCl_3(aq) + Zn_(s) → No Reaction

11. SrCl_2(aq) + CaS_(aq) → No Reaction

Worksheet 6 Reactions Practice Test 1

Simplify each and round off to the correct number of significant digits.

1. 19.239 + 5.37 24.61

2. 2.6699 - 1.27 1.40

3. 156.3 x 277.3 x 45.3 x 0.0445687 2.08

0.82569 x 19.235 x 2654

4. 9.66 x 10 ²⁴ x 5.37894 x 10^-15 x 4.532 x 10¹⁵ 3.98 x 10⁴¹

2.059 x 10 ^-20 5.343250 x 10¹⁵ 5.37894 x 10^-12

Convert using unit analysis

5. 627 g to mg

627 g x 1 x 10³ mg = 6.27 x 10⁵ g

1g

6. 4.05 x 10⁶ um to m

4.05 x 10⁶ μm x 1 m = 4.05 m

1 x 10⁶ μm

7. 8.148 ML to mL

8.148 ML x 1 x 10⁶ L x 1 x 10³ mL = 8.148 x 10⁹ mL

1ML 1L

8. 235.2 mg to Kg

235.2 mg x 1g x 1Kg = 2.352 x 10^-4 Kg

1 x 10³ mg 1 x 10³ g

9. 6.55 x 10¹⁴ mL to ML

6.55 x 10¹⁴ mL x 1 L x 1 ML = 6.55 x 10⁵ ML

1 x 10³ mL 1 x 10⁶ L

Complete, include all phase symbols, and balance each equation. Write formula, complete, and net ionic equations.

10. Ca_(s) + 2HOH_(l) → H_2(g) + Ca(OH)_2(s)

Ca_(s) + 2HOH_(l) → H_2(g) + Ca(OH)_2(s)

Ca_(s) + 2HOH_(l) → H_2(g) + Ca(OH)_2(s) Solids, liquids, and gases are not broken up.

11. 3ZnCl_2(aq) + 2Al_(s) → 3Zn_(s) + 2AlCl_3(aq)

3Zn²⁺_(aq) + 6Cl^-_(aq) + 2Al_(s) → 3Zn_(s) + 2Al³⁺_(aq) + 6Cl^-_(aq)

3Zn²⁺_(aq) + 2Al_(s) → 3Zn_(s) + 2Al³⁺_(aq)

12. SrCl_2(aq) + BaS_(aq) → No Reaction, both possible products are high solubility.

13. 2H₃PO_4(aq) + 3Ca(OH)_2(aq) → Ca₃(PO₄)_2(s) + 6HOH_(l)

6H⁺_(aq) + 2PO₄^3-_(aq) + 3Ca²⁺_(aq) + 6OH^-_(aq) → Ca₃(PO₄)_2(s) + 6HOH_(l)

6H⁺_(aq) + 2PO₄^3-_(aq) + 3Ca²⁺_(aq) + 6OH^-_(aq) → Ca₃(PO₄)_2(s) + 6HOH_(l)

14. 3Ba(NO₃)_2(aq) + 2Na₃PO_4(aq) → Ba₃(PO₄)_2(s) + 6NaNO_3(aq)

3Ba²⁺_(aq) + 6NO₃^-_(aq) + 6Na⁺_(aq) + 2PO₄^3-_(aq) → Ba₃(PO₄)_2(s) + 6Na⁺_(aq) + 6NO₃^-

3Ba²⁺_(aq) + 2PO₄^3-_(aq) → Ba₃(PO₄)_2(s)

15. 2AgNO_3(aq) + Na₂SO_4(aq) → Ag₂SO_4(s) + 2NaNO_3(aq)

2Ag⁺_(aq) + 2NO₃^-_(aq) + 2Na⁺_(aq) + SO₄^2-_(aq) → Ag₂SO_4(s) + 2Na⁺_(aq) + 2NO₃^-

2Ag⁺_(aq) + SO₄^2-_(aq) → Ag₂SO_4(s)

16. 2Fe(NO₃)_3(aq) + 3Zn_(s) → 2Fe_(s) + 3Zn(NO₃)_2(aq)

2Fe³⁺_(aq) + 6NO₃^-_(aq) + 3Zn_(s) → 2Fe_(s) + 3Zn²⁺_(aq) + 6NO₃^-_(aq)

2Fe³⁺_(aq) + 3Zn_(s) → 2Fe_(s) + 3Zn²⁺_(aq)

17. 2HCl_(aq) + CaCO_3(s) → CO_2(g) + CaCl_2(aq) + H₂O_(l)

2H⁺_(aq) + 2Cl^-_(aq) + CaCO_3(s) → CO_2(g) + Ca²⁺_(aq) + 2Cl^-_(aq) + H₂O_(l)

2H⁺_(aq) + CaCO_3(s) → CO_2(g) + Ca²⁺_(aq) + H₂O_(l)

Remember this one from the lab!

18. H₂SO_4(aq) + BaCO_3(s) →

H₂SO_4(aq) + BaCO_3(s) → CO_2(g) + BaSO_4(s) + H₂O_(l)

2H⁺_(aq) + SO₄^2-_(aq) + BaCO_3(s) → CO_2(g) + BaSO_4(s) + H₂O_(l)

2H⁺_(aq) + SO₄^2-_(aq) + BaCO_3(s) → CO_2(g) + BaSO_4(s) + H₂O_(l)

Remember this one from the lab!

Complete each formula equation only.

19. 2C₁₀H_22(l) + 31O_2(g) → 20CO_2(g) + 22H₂O_(l)

20. 2C₂₄H_46(l) + 71O_2(g) → 48CO_2(g) + 46H₂O_(l)

21. C₁₂H₂₂O_11(s) + 12O_2(g) → 12CO_2(g) + 11H₂O_(l)

22. Chlorine gas is bubbled into a solution of aluminum iodide.

3Cl_2(g) + 2AlI_3(aq) → 3I_2(g) + 2AlCl_3(aq)

23. Magnesium turnings are added to a solution of lead (II) chloride.

Mg_(s) + PbCl_2(aq) → Pb_(s) + MgCl_2(aq)

24. Barium metal is added to a solution of nitric acid.

Ba_(s) + 2HNO_3(aq) → H_2(g) + Ba(NO₃)_2(aq)

25. Lead II nitrate and Sodium chloride are mixed both in solution.

Pb(NO₃)_2(aq) + 2NaCl_(aq) → PbCl_2(s) + 2NaNO_3(aq)

26. Zinc bromide and Cesium hydroxide are mixed in solution.

ZnBr_2(aq) + 2CsOH_(aq) → Zn(OH)_2(s) + 2CsBr_(aq)

27. Zinc is reacted with phosphorus.

6Zn_(s) + P_4(s) → 2Zn₃P_2(s)

28. Iron (II) oxide liquid is decomposed by electrolysis.

2FeO_(l) → 2Fe_(s) + O_2(g)

29. Octane, C₈H₁₈, is burned as a fuel in cars.

2C₈H_18(l) + 25a_2(g) → 16CO_2(g) + 18H₂O_(l)

30.       A solid hydrocarbon that is 60.71 % C, 8.941 % H, and 30.35 % O undergoes a   reaction with a gas

            that reignites a glowing splint to produce a gas that turns limewater cloudy and a liquid that can cause

            rehydration. Write a balanced equation for this reaction.

C₈H₁₄O_3(s) + 10O_2(g) → 8CO_2(g) + 7H₂O_(l)

Worksheet # 7                       Reactions Practice 2                

Complete each reaction by writing a balanced equation. Include all phase symbols and balance all equations.  Name each reaction type in questions 1 – 7. Put in your workbook.

1.         4Ga_(s)     +         3O_2(g) → 2Ga₂O_{3 (s)}

Reaction Type                                     synthesis

 Δ

2.         2Ca₃P_2(s) → 6Ca _(s)  +  P_{4 (s)}

Reaction Type                                     decomposition

3.         K₂CO_3(s)          +          2HNO_3(aq) → 2KNO_{3 (aq)}    +    H₂O _(l)    +    CO_{2  (g)}

Reaction Type                                     acid-carbonate

4.         2C₁₂H_26(l)         +          37O_{2(g   )}→ 24 CO_{2 (g)}      +      26 H₂O _(l)

Reaction Type                                     combustion

5.         CaCl_2(aq)          +          BaS_(aq)  → CaS _(aq)    + BaCl_{2 (aq)}

Reaction Type                                     no reaction

6.         2Na_(s)     +          CaCl_2(aq) → Ca_(s) + 2NaCl_(aq)

Reaction Type                                    

7.         BaS_(aq)             +          ZnSO_4(aq) → BaSO_{4 (s)}     +       ZnS _(s)

Reaction Type                                     double replacement

8.         Write an equation to show what how Al₂(SO₄)_3(s) dissociates in water into ions.

Al₂(SO₄)_{3 (s)}    +    2Al³⁺_(aq)    +    3SO₄ ^2- _(aq)

9.        

Formula:         3Pb(NO₃)_2(aq)                +          2AlBr_3(aq) → 3PbBr_{2 (s)}  + 2Al(NO₃)_{3 (aq)}

Complete: 3Pb²⁺_(aq)  + 6NO₃^- _(aq) + 2Al³⁺_(aq) + 6Br ^– _(aq) + 3PbBr_{2 (s)}  + 2Al³⁺_(aq) + 6NO₃^- _(aq)

Net:                 Pb²⁺ _(aq)  +   2Br ^– _(aq) →    PbBr_{2 (s)}

10.      

Formula:         2Al_(s)                  +          3Cu(NO₃)_2(aq) → 2Al(NO₃)_{3 (aq)}  + 3Cu _(s)

Complete:       2Al_(s)      + 3Cu²⁺ _(aq) + 6NO₃^- _(aq)               →      2Al³⁺ _(aq) + 6NO₃^- _(aq) + 3Cu_(s)

Net:                 2Al_(s)      + 3Cu²⁺ _(aq)  →    2Al³⁺ _(aq) +  3Cu_(s)

11.      

Formula:         3Sr(OH)_2(aq)       +     Al₂(SO₄)_3(aq) → 2Al(OH)_{3 (s)}  + 3SrSO_{4 (s)}

Complete:       3Sr²⁺ _(aq)  + 6OH^- _(aq)  + 2Al³⁺ _(aq) + 3SO₄^2- _(aq)   →     2Al(OH)_{3 (s)}  + 3SrSO_{4 (s)}

Net:                  3Sr²⁺ _(aq)  + 6OH^- _(aq)  + 2Al³⁺ _(aq) + 3SO₄^2- _(aq) →     2Al(OH)_{3 (s)}  + 3SrSO_{4 (s)}

12.      

Formula:         2Na_(s)                 +          2H₂O_(l) → 2NaOH _(aq)   +     H_{2 (g)}

Complete:       2Na_(s)                +          2H₂O_(l) →    2Na⁺ _(aq)   +  2OH^- _(aq)   + H_{2 (g)}

Net:                 2Na_(s)                +          2H₂O_(l) →    2Na⁺ _(aq)   +  2OH^- _(aq)   + H_{2 (g)}

13.      

Formula:         3Sr(OH)_2(aq)       +     2H₃PO_4(aq) → 6HOH _(l)   +   Sr₃(PO4)_{2 (s)}

Complete:       3Sr²⁺ _(aq)  + 6OH^- _(aq)  +  6H⁺ _(aq) + 2PO4^3- _(aq) →   6HOH _(l)   +   Sr₃(PO₄)_{2 (s)}

Net:                 3Sr²⁺ _(aq)  + 6OH^- _(aq)  +  6H⁺ _(aq) + 2PO₄^3- _(aq) →   6HOH _(l)   +   Sr₃(PO₄)_{2 (s)}

14.      

Formula:         2HCl_(aq)      +     Na₂CO_3(s) → 2NaCl _(aq)  +  HOH _(l)  + CO_{2 (g)}

Complete:       2H⁺ _(aq)  + 2Cl^- _(aq) + Na₂CO_3(s) →   2Na⁺ _(aq) +  2Cl^- _(aq)  +  HOH _(l)  + CO_{2 (g)}

Net:                  2H⁺ _(aq)   + Na₂CO_3(s) →   2Na⁺ _(aq)  +  HOH _(l)  + CO_{2 (g)}

15.      

Formula:         2H₃PO_4(aq)      +     3MgCO_3(s) → Mg₃(PO₄)_{2 (s)}  +  3HOH _(l)  + 3CO_{2 (g)}

Complete:       6H⁺ _(aq)  + 2PO4^3- _(aq)  +    3MgCO_3(s) →  Mg₃(PO₄)_{2 (s)}  +  3HOH _(l)  + 3CO_{2 (g)}

Net:                 6H⁺ _(aq)  + 2PO4^3- _(aq)  +    3MgCO_3(s) →  Mg₃(PO₄)_{2 (s)}  +  3HOH _(l)  + 3CO_{2 (g)}

16.       2C₁₂H_26(l)    +    37O_2(g) → 24CO_{2 (g)}   +    26H₂0 _(g)

17.       C₂₆H_52(l)    +    39O_2(g) →  26CO_{2 (g)}   +    26H₂0 _(g)

18.       A container of copper (II) oxide has been accidentally contaminated with copper (I) oxide.

            The total mass of both oxides is 9.55 g. Through a single replacement reaction with Zn, the copper

            was able to be purified and was found to have a mass of 8.42 g. What was the original masses of

            the copper (II) and copper (I) oxides before they were mixed?

A g Cu₂O   x    1mol     x   2 mol Cu      x    63.5 g     =     0.8881 A g Cu

                          143.0 g      1 mol Cu₂O       1 mole

(9.55 – A)g CuO    x   1mol    x   1 mol Cu   x   63.5 g    =    7.628  -  0.7987 A g Cu

                                     79.5 g       1 mol CuO     1 mole

0.8881 A g Cu   +    7.628    -    0.7987 A g Cu         =   total grams Cu

0.0894 A  +     7.628     =   total grams Cu

Grams Cu                   =          Grams Cu

0.0894 A  + 7.628       =          8.42

0.0894 A                     =          0.792

A         =          8.869

A         =          mass Cu₂O      =          8.86 g 

9.55 –  A       =          mass CuO       =          0.69 g

Worksheet # 8                       Reactions Practice Test 3                

Complete each reaction by writing a balanced equation. Include all phase symbols and balance all equations.  Name each reaction type in questions 1 – 7. Put in your workbook.

1.         4 Al_(s)   +          P_4(g) →        4 AlP_(s)

Reaction Type    Synthesis

 Δ

2.         4 Ga₃S_2(s) →        12 Ga_(s)   +    S_8(s)

Reaction Type   Decomposition

3.         CaCO_3(s)         +          2 HCl_(aq) →    CO₂    +    CaCl_2(aq)      +     H₂O_(l)

Reaction Type   Acid Carbonate

4.         C₁₄H_30(l)          +          21.5 O_2(g) →    14 CO_2(g)      +   15 H₂O_(l)

Reaction Type Combustion

5.         SrCl_2(aq)           +          BaS_(aq) →        No Reaction

Reaction Type No Reaction

6.         2K_(s)     +          CaCl_2(aq) →    2KCl_(aq)      +    Ca_(s)

Reaction Type Single Replacement

7.         BaS_(aq)           +          ZnSO_4(aq) →   BaSO_4(s)    +   ZnS_(s)

Reaction Type Double Replacement

8.         Write an equation to show what how Ga₂(CO₃)_3(s) dissociates in water into ions.

Ga₂(CO₃)_3(s)     →   2Ga³⁺_(aq)    +   3CO₃^2-_(aq)

9.        

Formula:         3Pb(NO₃)_2(aq)               +          2GaCl_3(aq) →        3PbCl_2(s)    +    2Ga(NO₃)_3(aq)

Complete:       3Pb²⁺_(aq)   + 6NO₃^-_(aq) + 2Ga³⁺_(aq)   + 6Cl^-_(aq)  →  3PbCl_2(s)   +  2Ga²⁺_(aq) + 6NO₃^-_(aq)

Net:                 3Pb²⁺_(aq)   +   6Cl^-_(aq)   →      3PbCl_2(s)

10.      

Formula:         Zn_(s)                    +          Cu(NO₃)_2(aq) →   Zn(NO₃)_2(aq)      +    Cu_(s)

Complete:       Zn _(s)   + Cu²⁺_(aq)    +  2NO₃^-_(aq)   →   Zn²⁺_(aq)   + 2NO₃^-_(aq)    +   Cu_(s)

Net:                 Zn _(s)   + Cu²⁺_(aq)   →   Zn²⁺_(aq)   +   Cu_(s)

11.      

Formula:         3Sr(OH)_2(aq)      +     Al₂(SO₄)_3(aq) →              3SrSO_4(s)    +   2Al(OH)_3(s)

Complete:       3Sr²⁺_(aq)    +    6OH^-_(aq)    +    Al³⁺_(aq)   3SO₄^2-_(aq)  →     3SrSO_4(s)    +   2Al(OH)_3(s)

Net:                 3Sr²⁺_(aq)    +    6OH^-_(aq)    +    Al³⁺_(aq)   3SO₄^2-_(aq)  →     3SrSO_4(s)    +   2Al(OH)_3(s)

12.      

Formula:         Ca_(s)                    +          2 H₂O_(l) →   Ca(OH)_2(s)                             + H_2(g)

Complete:       Ca_(s)                    +         2 H₂O_(l) →  Ca(OH)_2(s) +  H_2(g)

Net:                 Ca_(s)                    +         2 H₂O_(l) →  Ca(OH)_2(s) + H_2(g)

13.      

Formula:         3Ba(OH)_2(aq)    +     2H₃PO_4(aq) →   Ba₃(PO₄)_2(s)    +  6H₂O_(l)

Complete:       3Ba²⁺_(aq)   +  6OH^-_(aq)    + 6H⁺_(aq) +   2PO₄^3-_(aq)  →  Ba₃(PO₄)_2(s)    +  6H₂O_(l)

Net:                 3Ba²⁺_(aq)   +  6OH^-_(aq)    + 6H⁺_(aq) +   2PO₄^3-_(aq)  →  Ba₃(PO₄)_2(s)    +  6H₂O_(l)

14.      

Formula:         H₂SO_4(aq)      +     Na₂CO_3(s) →  Na₂SO_4(aq)   + H₂O_(l)   +  CO_2(g)

Complete:       2H⁺_(aq)   +   SO₄^2-_(aq)   +   Na₂CO_3(s) →  2Na⁺_(aq)   +  SO₄^2-_(aq)  + H₂O_(l)   +  CO_2(g)

Net:                 2H⁺_(aq)   +  Na₂CO_3(s) →  2Na⁺_(aq)   +  H₂O_(l)   +  CO_2(g)

15.       9.000 g of a mixture of Fe₃S₂ and FeS are reduced to 5.1252 g of pure Fe.

What is are masses of the Fe₃S₂ and FeS in the original mixture?

A g Fe₂S₃   x    1mol     x   2 mol Fe      x    55.8 g     =     0.53679 A g Fe

                         207.9 g      1 mol Fe₂S₃       1 mole

(9.000 – A)g FeS    x   1mol    x   1 mol Fe   x   55.8 g    =    5.71331  -  0.63481 A g Fe

                                   87.9 g       1 mol FeS     1 mole

0.53679 A g Fe +    5.71331  -  0.63481 A g Fe =   total grams Fe

-0.09802 A  +     5.71331  =   total grams Fe

Grams Fe                   =          Grams Fe

-0.09802 A  +     5.71331  =          5.1252

-0.09802 A  =          -0.58811

A       =          6.00

A         =          mass Fe₂S₃ =          6.00 g 

9.000 –  A       =          mass Fe =          3.00 g