Chapter 5

Mixing each of the following salt solutions results in the formation of a precipate. In each case, identify the insoluble salt. a. \(\mathrm{NaCl}+\mathrm{Pb}\left(\mathrm{NO}_{3}\right) 2\) b. \(\mathrm{Fe}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right) 3+\mathrm{KOH}\) c. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{K}_{2} \mathrm{SO}_{4}\) d. \(\mathrm{Li}_{2} \mathrm{~S}+\mathrm{CuSO}_{4}\) e. \(\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}+\mathrm{LiOH}\)

Write a balanced chemical equation for the reactions given below: a. When hydrogen gas reacts is combined with oxygen gas and the mixture ignited with a spark, water is formed in a violent reaction. b. Lead (IV) oxide reacts with HCl to give lead (II) chloride, chlorine gas and water. c. Solid potassium chlorate decomposes on heating to form solid KCl and oxygen gas.

Arsonic and nitric acids react to form nitrogen monoxide, arsenic acid and water according to the equation shown below. Is this an example of a redox reaction? \(2 \mathrm{HNO}_{3}(a q)+3 \mathrm{H}_{3} \mathrm{AsO}_{3}(a q) \rightarrow 2 \mathrm{NO}(g)+3 \mathrm{H}_{3} \mathrm{AsO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})\)

a. Write a chemical equation for the reaction of solid iron with solid sulfur to form solid iron(II) sulfide. b. Write a chemical equation for the reaction of solid carbon with solid magnesium oxide to form carbon monoxide gas and magnesium metal.

For each of the reactions given below, calculate the oxidation number of each of the elements in the reactants and the products and determine if the reaction involves oxidation-reduction. If it is a redox reaction, identify the elements that have been oxidized and reduced. a. \(\mathrm{Cu}_{2} \mathrm{~S} \rightarrow 2 \mathrm{Cu}+\mathrm{S}\) Reactants: Cu ___________ \(\mathrm{S}\) ___________ Products: Cu ___________ \(\mathrm{S}\) ___________ Element oxidized: ___________ Element Reduced ___________ b. \(\mathrm{CaCO}_{3} \rightarrow \mathrm{CaO}+\mathrm{CO}_{2}\) Reactants: Ca ___________ C ___________ O ___________ Products: \(\mathrm{Ca}\) ___________ \(C\) ___________ O ___________ Element oxidized: ___________ Element Reduced ___________ c. \(\mathrm{Fe}_{2} \mathrm{O}_{3}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{Fe}+3 \mathrm{H}_{2} \mathrm{O}\) Reactants: Fe ___________ O ___________ \(\mathrm{H}\) ___________ Products: Fe ___________ O ___________ \(\mathrm{H}\) ___________ Element oxidized: ___________ Element Reduced ___________ \(\mathrm{d} . \mathrm{AgNO}_{3}+\mathrm{NaCl} \rightarrow \mathrm{AgCl}(\mathrm{s})+\mathrm{NaNO}_{3}\) Reactants: Ag ___________ \(\mathrm{N}\) ___________ \(\mathrm{O}\) ___________ \(\mathrm{Na}\) ___________ \(\mathrm{Cl}\) ___________ Products: \(\mathrm{Ag} \) ___________ \( \mathrm{N}\) ___________ \( \mathrm{O}\) ___________ \( \mathrm{Na}\) ___________ Element oxidized: ___________ Element Reduced ___________