Chapter 9

When carbon monoxide and oxygen react, carbon dioxide forms. $$ \text { carbon monoxide } (\mathrm {g})+ \text { oxygen }(\mathrm {g}) \rightarrow \text { carbon dioxide } (\mathrm {g})$$

Challenge Write the word equation and the skeleton equation for the following reaction: when heated, solid potassium chlorate yields solid potassium chloride and oxygen gas.

In water, iron(III) chloride reacts with sodium hydroxide, producing solid iron(III) hydroxide and sodium chloride.

Liquid carbon disulfide reacts with oxygen gas, producing carbon dioxide gas and sulfur dioxide gas.

Challenge A piece of zinc metal is added to a solution of hydroge sulfate. This reaction produces a gas and a solution of zinc sulfate.

A Explain why it is important that a chemical equation be balance

List three types of physical evidence that indicate a chemical reaction has occurred.

Compare and contrast a skeleton equation and a chemical equation.

Explain why it is important to reduce coefficients in a balanced equation to the lowest-possible whole-number ratio.

Analyze When balancing a chemical equation, can you adjust the subscript in a formula? Explain.

Assess Is the following equation balanced? If not, correct the coefficients to balance the equation. $$2 \mathrm{K}_{2} \mathrm{CrO}_{4}(\mathrm{aq})+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{KNO}_{3}(\mathrm{aq})+\mathrm{Pb} \mathrm{CrO}_{4}(\mathrm{s})$$

Evaluate Aqueous phosphoric acid and aqueous calcium hydroxide react to form solid calcium phosphate and water. Write a balanced chemical equation for this reaction.

The solids aluminum and sulfur react to produce aluminum sulfide.

Water and dinitrogen pentoxide gas react to produce aqueous hydrogen nitrate.

The gases nitrogen dioxide and oxygen react to produce dinitrogen pentoxide gas.

Challenge Sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) and sodium hydroxide solutions react to produce aqueous sodium sulfate and water.

Aluminum oxide(s) decomposes when electricity passes through it.

Nickel( II) hydroxide(s) decomposes to produce nickel( II) oxide(s) and water.

Aqueous barium chloride and aqueous potassium carbonate react to produce solid barium carbonate and aqueous potassium chloride.

Aqueous sodium oxalate and aqueous lead(II) nitrate react to produce solid lead(II) oxalate and aqueous sodium nitrate.

Challenge Acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) and potassium hydroxide react to produce potassium acetate and water.

Describe the four types of chemical reactions and their characteristics.

Explain how an activity series of metals is organized.

Compare and contrast single-replacement reactions and double-replacement reactions.

Describe the result of a double-replacement reaction.

Classify What type of reaction is most likely to occur when barium reacts with fluorine? Write the chemical equation for the reaction.

Interpret Data Could the following reaction occur? Explain your answer. $$3 \mathrm{Ni}+2 \mathrm{AuBr}_{3} \rightarrow 3 \mathrm{NiBr}_{2}+2 \mathrm{Au}$$

Aqueous solutions of potassium iodide and silver nitrate are mixed, forming the precipitate silver iodide.

Aqueous solutions of ammonium phosphate and sodium sulfate are mixed. No precipitate forms and no gas is produced.

Aqueous solutions of aluminum chloride and sodium hydroxide are mixed, forming the precipitate aluminum hydroxide.

Aqueous solutions of lithium sulfate and calcium nitrate are mixed, forming the precipitate calcium sulfate.

Challenge When aqueous solutions of sodium carbonate and manganese(V) chloride are mixed, a precipitate forms. The precipitate is a compound containing manganese.

Mixing sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) and aqueous potassium hydroxide produces water and aqueous potassium sulfate.

Mixing hydrochloric acid (HCl) and aqueous calcium hydroxide produces water and aqueous calcium chloride.

Mixing nitric acid (HNO \(_{3} )\) and aqueous ammonium hydroxide produces water and aqueous ammonium nitrate.

Challenge When benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) and magnesium hydroxide are mixed, water and magnesium benzoate are produced.

Sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{\mathrm{A}}\right)\) reacts with aqueous sodium cyanide, forming hydrogen cyanide gas and aqueous sodium sulfate.

Challenge Aqueous potassium iodide reacts with lead nitrate in solution, forming solid lead iodide.

List three common types of products produced by reactions that occur in aqueous solutions.

Describe solvents and solutes in an aqueous solution.

Distinguish between a complete ionic equation and a net ionic equation.

Write complete ionic and net ionic equations for the reaction between sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) and calcium carbonate \(\left(\mathrm{CaCO}_{3}\right)\). $$\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{s}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{CaSO}_{4}(\mathrm{aq})$$

Analyze Complete and balance the following equation $$\mathrm{CO}_{2}(\mathrm{g})+\mathrm{HCl}(\mathrm{aq}) \rightarrow$$

Predict What type of product would the following reaction be most likely to produce? Explain your reasoning. $$\mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow$$

Formulate Equations A reaction occurs when nitric acid (HNO \(_{3}\) ) is mixed with an aqueous solution of potassium hydrogen carbonate. Aqueous potassium nittrate is produced. Write the chemical and net ionic equations for the reaction.

Define chemical equation.

Distinguish between a chemical reaction and a chemical equation.

Explain the difference between reactants and products.

What do the arrows and coefficients in equations communicate?

Does a conversion of a substance into a new substance always indicate that a chemical reaction has occurred? Explain.