Balancing Equations Worksheet and Key

Balancing Equations Worksheet and Key 1. Answer the following questions about the chemical equation shown below: 2 H2 + O2 → 2 H2O a) What are the reactants? b) What is the product? c) What do we call the number "2" in front of the H2 (and H2O)? d) Is the reaction balanced? e) Why is there not a coefficient for O2? . f) How many hydrogen atoms are needed to produce two H2O molecules? g) How many oxygen atoms are needed to produce two H2O molecules? h) How many hydrogen molecules are needed to produce two H2O molecules? i) How many oxygen molecules are needed to produce two H2O molecules? j) Write the "word equation" that you would use to describe this reaction. • Use words in a sentence, not formulas or an arrow. Ignore the coefficients. 2. Balance the following chemical equations: a) Fe + O2 → Fe2O3 b) H2 + Cl2 → HCl c) Ag + H2 S → → Ag2S + H2 d) CH4 + O2 e) HgO → f) Co + H2O → Co2O3 + H2 Hg + CO2 + H2O O2 3. Write balanced chemical equations for each of the following descriptions of a chemical reaction. • You do not need to include the phases of the reactants or products. IMPORTANT NOTE: Before attempting to balance the equations, you must first convert the compound names into the correct chemical formulas. If you begin to struggle with that, you may wish to go back to Chapter 3 and re-work the naming problems. a) Aluminum metal reacts with copper(II) chloride to produce aluminum chloride and copper metal. b) Lead(II) nitrate reacts with sodium bromide to produce lead(II) bromide and sodium nitrate. • HINT: Since you have the same polyatomic ion (nitrate) on both sides of the equation you can use the shortcut that was listed in Step #1 of our balancing method. c) Zinc metal reacts with oxygen gas to produce zinc oxide (Recall that oxygen is one of the diatomic molecules that are referred to by their element's name). d) Aluminum sulfate reacts with barium iodide to produce aluminum iodide and barium sulfate. e) At temperatures reached during baking, sodium bicarbonate (baking soda) decomposes (reacts) to produce sodium carbonate, carbon dioxide, and dihydrogen monoxide. • Recall that bicarbonate is a polyatomic ion (not the same as the carbonate polyatomic ion). f) Sodium metal reacts with water to produce sodium hydroxide and hydrogen gas. g) Lead(IV) sulfide reacts with oxygen gas to produce lead(IV) oxide and sulfur dioxide. h) Zinc metal reacts with phosphoric acid to produce zinc phosphate and hydrogen gas. (NOTE: the formula of phosphoric acid is H3PO4) SEE NEXT PAGE FOR THE ANSWER KEY ANSWER KEY 1. Answer the following questions about the chemical equation shown below: 2 H2 + O2 → 2 H2O a) What are the reactants? H2 and O2 b) What is the product? H2O c) What is the number "2" in front of the H2 (and H2O) called? Coefficient d) Is the reaction balanced? Yes e) Why is there not a coefficient in for O2? When the coefficient would be "1", it is omitted. f) How many hydrogen atoms are needed to produce two H2O molecules? 4 g) How many oxygen atoms are needed to produce two H2O molecules? 2 h) How many hydrogen molecules are needed to produce two H2O molecules? 2 i) How many oxygen molecules are needed to produce two H2O molecules? 1 j) Write the "word equation" that you would use to describe this reaction. • Use words in a sentence, not formulas or an arrow. Ignore the coefficients. Hydrogen reacts with oxygen to produce dihydrogen monoxide (or water). or Hydrogen plus oxygen produces dihydrogen monoxide (or water). o You can write "forms" instead of "produces" 2. Balance the following chemical equations: a) 4 Fe + 3 O2 → b) H2 + Cl2 → 2 HCl c) 2 Ag + H2S → 2 Fe2O3 Ag2S + H2 d) CH4 + 2 O2 → CO2 + 2 H2O e) 2 HgO → f) 2 Co + 3 H2O → Co2O3 + 3 H2 2 Hg + O2 3. Write balanced chemical equations for each of the following descriptions of a chemical reaction. • You do not need to include the phases of the reactants or products. IMPORTANT NOTE: Before attempting to balance the equations, you must first convert the compound names into the correct chemical formulas. If you begin to struggle with that, you may wish to go back to Chapter 3 and re-work the naming problems. a) Aluminum metal reacts with copper(II) chloride to produce aluminum chloride and copper metal. 2 Al + 3 CuCl2 → 2 AlCl3 + 3 Cu b) Lead(II) nitrate reacts with sodium bromide to produce lead(II) bromide and sodium nitrate. • HINT: Since you have the same polyatomic ion (nitrate) on both sides of the equation you can use the shortcut that was listed in Step #1 of our balancing method. Pb(NO3)2 + 2 NaBr → PbBr2 + 2 NaNO3 c) Zinc metal reacts with oxygen gas to produce zinc oxide (Recall that oxygen is one of the diatomic molecules that are referred to by their element's name). 2 Zn + O2 → 2 ZnO d) Aluminum sulfate reacts with barium iodide to produce aluminum iodide and barium sulfate. Al2(SO4)3 + 3 BaI2 → 2 AlI3 + 3 BaSO4 e) At temperatures reached during baking, sodium bicarbonate (baking soda) decomposes (reacts) to produce sodium carbonate, carbon dioxide, and dihydrogen monoxide. • Recall that bicarbonate is a polyatomic ion (not the same as the carbonate polyatomic ion). 2 NaHCO3 → Na2CO3 + CO2 + H2O f) Sodium metal reacts with water to produce sodium hydroxide and hydrogen gas. 2 Na + 2 H2O → 2 NaOH + H2 g) Lead(IV) sulfide reacts with oxygen gas to produce lead(IV) oxide and sulfur dioxide. PbS2 + 3 O2 → PbO2 + 2 SO2 h) Zinc metal reacts with phosphoric acid to produce zinc phosphate and hydrogen gas. (NOTE: the formula of phosphoric acid is H3PO4) 3 Zn + 2 H3PO4 → Zn3(PO4)2 + 3 H2 about:blank 4/4