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7.E: Introduction to Chemical Reactions (Exercises)

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    5.1: The Law of Conservation of Matter

    1. What is the law of conservation of matter?
    2. How does the law of conservation of matter apply to chemistry?

    AnswerS

    1. The law of conservation of matter states that in any given system that is closed to the transfer of matter, the amount of matter in the system stays constant
    2. The law of conservation of matter says that in chemical reactions, the total mass of the products must equal the total mass of the reactants.

    Exercises

    1. Express the law of conservation of matter in your own words.

    2. Explain why the concept of conservation of matter is considered a scientific law.

    3. Potassium hydroxide (\(\ce{KOH}\)) readily reacts with carbon dioxide (\(\ce{CO2}\)) to produce potassium carbonate (\(\ce{K2CO3}\)) and water (\(\ce{H2O}\)). How many grams of potassium carbonate is produced if 224.4 g of \(\ce{KOH}\) reacted with 88.0 g of \(\ce{CO2}\). The reaction also produced 36.0 g of water.

    Answers

    1. Matter may not be created or destroyed.

    2. The concept is a scientific law because it is based on experimentation.

    3. 276.4 g

    5.2: Chemical Equations

    Concept Review Exercises

    1. What are the parts of a chemical equation?
    2. Explain why chemical equations need to be balanced.

    Answers

    a. reactants and products

    b. Chemical equations need to be balanced to satisfy the law of conservation of matter.

    Exercises

    1. Write a chemical equation to express the fact that hydrogen gas and solid iodine react to make gaseous hydrogen iodide. Make sure the equation satisfies the law of conservation of matter.

    2. Write a chemical equation to express the fact that sodium metal and chlorine gas react to make solid sodium chloride. Make sure the equation satisfies the law of conservation of matter.

    3. Write an equation expressing the fact that hydrogen gas and fluorine gas react to make gaseous hydrogen fluoride. Make sure the equation satisfies the law of conservation of matter.

    4. Write an equation expressing the fact that solid potassium and fluorine gas react to make solid potassium fluoride. Make sure the equation satisfies the law of conservation of matter.

    5. Mercury reacts with oxygen to make mercury(II) oxide. Write a balanced chemical equation that summarizes this reaction.

    6. Octane (C8H18) reacts with oxygen to make carbon dioxide and water. Write a balanced chemical equation that summarizes this reaction.

    7. Propyl alcohol (C3H7OH) reacts with oxygen to make carbon dioxide and water. Write a balanced chemical equation that summarizes this reaction.

    8. Sulfuric acid (H2SO4) reacts with iron metal to make iron(III) sulfate and hydrogen gas. Write a balanced chemical equation that summarizes this reaction.

    9. Balance each equation.

      1. MgCl2 + K → KCl + Mg
      2. C6H12O6 + O2 → CO2 + H2O
      3. NaN3 → Na + N2 (This is the reaction used to inflate airbags in cars.)

    10. Balance each equation.

      1. NH4NO3 → N2O + H2O
      2. TiBr4 + H2O → TiO2 + HBr
      3. C3H5N3O9 → CO2 + N2 + O2 + H2O (This reaction represents the decomposition of nitroglycerine.)

    11. Balance each equation.

      1. NH3 + O2 → NO + H2O
      2. Li + N2 → Li3N
      3. AuCl → Au + AuCl3

    12. Balance each equation.

      1. NaOH + H3PO4 → Na3PO4 + H2O
      2. N2H4 + Cl2 → N2 + HCl
      3. Na2S + H2S → NaSH

    13. Chromium(III) oxide reacts with carbon tetrachloride to make chromium(III) chloride and phosgene (COCl2). Write the balanced chemical equation for this reaction.

    14. The reaction that occurs when an Alka-Seltzer tablet is dropped into a glass of water has sodium bicarbonate reacting with citric acid (H3C6H5O7) to make carbon dioxide, water, and sodium citrate (Na3C6H5O7). Write the balanced chemical equation for this reaction.

    15. When sodium hydrogen carbonate is used to extinguish a kitchen fire, it decomposes into sodium carbonate, carbon dioxide and water. Write a balanced chemical equation for this reaction.

    16. Elemental bromine gas can be generated by reacting sodium bromide with elemental chlorine. The other product is sodium chloride. Write a balanced chemical equation for this reaction.

    Answers

    1. H2(g) + I2(s) → 2HI(g)

    2. 2Na(s) + Cl2(g) → 2NaCl(s)

    1. H2(g) + F2(g) → 2HF(g)

    4. 2K(s) + F2(g) → 2KF(s)

    1. 2Hg + O2 → 2HgO

    6. 2C8H18 + 25O2 → 16CO2 + 18H2O

    1. 2C3H7OH + 9O2 → 6CO2 + 8H2O

    8. 3H2SO4 + 2Fe → Fe2(SO4)3 + 3H2
      1. MgCl2 + 2K → 2KCl + Mg
      2. C6H12O6 + 6O2 → 6CO2 + 6H2O
      3. 2NaN3 → 2Na + 3N2

    10.

    1. NH4NO3 → N2O + 2H2O
    2. TiBr4 + 2H2O → TiO2 + 4HBr
    3. 4C3H5N3O9 → 12CO2 + 6N2 + O2 + 10H2O

    11.

    1. 4NH3 + 5O2 → 4NO + 6H2O
    2. 6Li + N2 → 2Li3N
    3. 3AuCl → 2Au + AuCl3

    12.

    1. 3NaOH + H3PO4 → Na3PO4 + 3H2O
    2. N2H4 + 2Cl2 → N2 + 4HCl
    3. Na2S + H2S → 2NaSH

    13. Cr2O3 + 3CCl4 → 2CrCl3 + 3COCl2

    14. 3NaHCO3 + H3C6H5O7 → 3CO2 + 3H2O + Na3C6H5O7

    15. 2NaHCO3 → Na2CO3 + CO2 + H2O

    16. 2NaBr + Cl2 → Br2 + 2NaCl

    5.3: Quantitative Relationships Based on Chemical Equations

    Concept Review Exercises

    1. Explain how stoichiometric ratios are constructed from a chemical equation.
    2. Why is it necessary for a chemical equation to be balanced before it can be used to construct conversion factors?

    Answers

    1. Stoichiometric ratios are made using the coefficients of the substances in the balanced chemical equation.
    2. A balanced chemical equation is necessary so one can construct the proper stoichiometric ratios.

    Exercises

    1. Balance this equation and write every stoichiometric ratio you can from it.

      NH4NO3 → N2O + H2O

    2. Balance this equation.

      N2 + H2 → NH3

    3. Balance this equation and write every stoichiometric ratio you can from it.

      Fe2O3 + C → Fe + CO2

    4. Balance this equation.

      Fe2O3 + CO → Fe + CO2

    5. Balance this equation and determine how many molecules of CO2 are formed if 15 molecules of C6H6 are reacted.

      C6H6 + O2 → CO2 + H2O

    6. Balance this equation and determine how many formula units of Ag2CO3(s) are produced if 20 formula units of Na2CO3 are reacted.

      Na2CO3(aq) + AgNO3(aq) → NaNO3(aq) + Ag2CO3(s)

    7. Copper metal reacts with nitric acid according to this equation:

      3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(ℓ)

      1. Verify that this equation is balanced.
      2. How many Cu atoms will react if 488 molecules of aqueous HNO3 are reacted?

    8. Gold metal reacts with a combination of nitric acid and hydrochloric acid according to this equation:

      Au(s) + 3HNO3(aq) + 4HCl(aq) → HAuCl4(aq) + 3NO2(g) + 3H2O(ℓ)

      1. Verify that this equation is balanced.
      2. How many Au atoms react with 639 molecules of aqueous HNO3?

    9. Sulfur can be formed by reacting sulfur dioxide with hydrogen sulfide at high temperatures according to this equation:

      SO2(g) + 2H2S(g) → 3S(g) + 2H2O(g)

      1. Verify that this equation is balanced.
      2. How many S atoms will be formed from by reacting 1,078 molecules of H2S?

    10. Nitric acid is made by reacting nitrogen dioxide with water:

      3NO2(g) + H2O(ℓ) → 2HNO3(aq) + NO(g)

      1. Verify that this equation is balanced.
      2. How many molecules of NO will be formed by reacting 2,268 molecules of NO2?

    Answers

    1. NH4NO3 → N2O + 2H2O; the stoichiometric ratios are \(\mathrm{\dfrac{1NH_4NO_3}{1N_2O}\:,\: \dfrac{1NH_4NO_3}{2H_2O}\:,\: \dfrac{1N_2O}{2H_2O}\:,}\) and their reciprocals.

    2. N2 + 3H2 → 2NH3

    1. 2Fe2O3 + 3C → 4Fe + 3CO2; the stoichiometric ratios are \(\mathrm{\dfrac{2Fe_2O_3}{3C}\:,\: \dfrac{2Fe_2O_3}{4Fe}\:,\: \dfrac{2Fe_2O_3}{3CO_2}\:,\: \dfrac{3C}{4Fe}\:,\: \dfrac{3C}{3CO_2}\:,\: \dfrac{4Fe}{3CO_2}\:,\: }\) and their reciprocals.

    4. Fe2O3 + 3CO → 2Fe + 3CO2

    1. 2C6H6 + 15O2 → 12CO2 + 6H2O; 90 molecules

    6. Na2CO3(aq) + 2AgNO3(aq) → 2NaNO3(aq) + Ag2CO3(s); 20 formula units

    7.

    1. It is balanced.
    2. 183 atoms

    8.

    1. It is balanced.
    2. 213 atoms

    9.

    1. It is balanced.
    2. 1,617 atoms
    10.
    1. It is balanced.
    2. 756 molecules

    5.4: Some Types of Chemical Reactions

    Concept Review Exercises

    1. What is the difference between a combination reaction and a combustion reaction?
    2. Give the distinguishing characteristic(s) of a decomposition reaction.
    3. How do we recognize a combustion reaction?

    Answers

    1. A combination reaction produces a certain substance; a combustion reaction is a vigorous reaction, usually a combination with oxygen, that is accompanied by the production of light and/or heat.
    2. In a decomposition reaction, a single substance reacts to make multiple substances as products.
    3. A combustion reaction is typically a vigorous reaction accompanied by light and/or heat, usually because of reaction with oxygen.

    Exercises

    1. Identify each type of reaction.

      1. C6H5CH3 + 9O2 → 7CO2 + 4H2O
      2. 2NaHCO3 → Na2CO3 + H2O + CO2
      3. C + 2H2 → CH4

    2. Identify each type of reaction.

      1. P4O10 + 6H2O → 4H3PO4
      2. FeO + SO3 → FeSO4
      3. CaCO3(s) → CO2(g) + CaO(s)

    3. Identify each type of reaction.

      1. 2NH4NO3(s) → 2N2(g) + 4H2O(g) + O2(g)
      2. Hg(ℓ) + ½O2 (g) → HgO(s)
      3. CH2CH2(g) + Br2(ℓ) → CH2BrCH2Br

    4. Identify each type of reaction.

      1. Ti(s) + O2(g) → TiO2(s)
      2. H2SO3(aq) → H2O(ℓ) + SO2(g)
      3. 3O2(g) → 2O3(g)

    Answers

    1.

    a. combustion

    b. decomposition

    c. combination

    2.

    a. combination

    b. combination

    c. decomposition

    3.

    a. decomposition

    b. combustion (also combination)

    c. combination

    4.

    a. combination

    b. decomposition

    c. combination

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