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Chapter 3: Problem 13

Write balanced chemical equations to correspond to each of the following descriptions: (a) Solid calcium carbide, \(\mathrm{CaC}_{2}\), reacts with water to form an aqueous solution of calcium hydroxide and acetylene gas, \(\mathrm{C}_{2} \mathrm{H}_{2}\). (b) When solid potassium chlorate is heated, it decomposes to form solid potassium chloride and oxygen gas. (c) Solid zinc metal reacts with sulfuric acid to form hydrogen gas and an aqueous solution of zinc sulfate. (d) When liquid phosphorus trichloride is added to water, it reacts to form aqueous phosphorous acid, \(\mathrm{H}_{3} \mathrm{PO}_{3}(a q),\) and aqueous hydrochloric acid. (e) When hydrogen sulfide gas is passed over solid hot iron(III) hydroxide, the resultant reaction produces solid iron(III) sulfide and gaseous water.

Short Answer

Expert verified
Here are the balanced chemical equations for the given reactions: (a) CaC2(s) + 2H2O(l) -> Ca(OH)2(aq) + C2H2(g) (b) 2KClO3(s) -> 2KCl(s) + 3O2(g) (c) Zn(s) + H2SO4(aq) -> H2(g) + ZnSO4(aq) (d) PCl3(l) + 3H2O(l) -> H3PO3(aq) + 3HCl(aq) (e) 3H2S(g) + 2Fe(OH)3(s) -> Fe2S3(s) + 6H2O(g)

Step by step solution

01

(a) Reaction between calcium carbide and water

Reactants: Solid calcium carbide (CaC2) and water (H2O) Products: Aqueous calcium hydroxide (Ca(OH)2) and acetylene gas (C2H2) Unbalanced equation: CaC2(s) + H2O(l) -> Ca(OH)2(aq) + C2H2(g) To balance the equation, we need 2 water molecules for every calcium carbide: Balanced equation: CaC2(s) + 2H2O(l) -> Ca(OH)2(aq) + C2H2(g)
02

(b) Decomposition of potassium chlorate

Reactants: Solid potassium chlorate (KClO3) Products: Solid potassium chloride (KCl) and oxygen gas (O2) Unbalanced equation: KClO3(s) -> KCl(s) + O2(g) To balance the equation, we need 2 potassium chlorate molecules for every 3 oxygen molecules: Balanced equation: 2KClO3(s) -> 2KCl(s) + 3O2(g)
03

(c) Reaction between zinc and sulfuric acid

Reactants: Solid zinc (Zn) and sulfuric acid (H2SO4) Products: Hydrogen gas (H2) and aqueous zinc sulfate (ZnSO4) Unbalanced equation: Zn(s) + H2SO4(aq) -> H2(g) + ZnSO4(aq) This equation is already balanced.
04

(d) Reaction between phosphorus trichloride and water

Reactants: Liquid phosphorus trichloride (PCl3) and water (H2O) Products: Aqueous phosphorous acid (H3PO3) and aqueous hydrochloric acid (HCl) Unbalanced equation: PCl3(l) + H2O(l) -> H3PO3(aq) + HCl(aq) To balance the equation, we need 3 hydrochloric acid molecules for every phosphorus trichloride molecule: Balanced equation: PCl3(l) + 3H2O(l) -> H3PO3(aq) + 3HCl(aq)
05

(e) Reaction between hydrogen sulfide and iron(III) hydroxide

Reactants: Hydrogen sulfide gas (H2S) and solid hot iron(III) hydroxide (Fe(OH)3) Products: Solid iron(III) sulfide (Fe2S3) and gaseous water (H2O) Unbalanced equation: H2S(g) + Fe(OH)3(s) -> Fe2S3(s) + H2O(g) To balance the equation, we need 3 hydrogen sulfide molecules and 2 iron(III) hydroxide molecules for every 2 iron(III) sulfide molecules and 6 water molecules: Balanced equation: 3H2S(g) + 2Fe(OH)3(s) -> Fe2S3(s) + 6H2O(g)

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Most popular questions from this chapter

(a) What is the mass, in grams, of a mole of \({ }^{12} \mathrm{C} ?\) (b) How many carbon atoms are present in a mole of \({ }^{12} \mathrm{C} ?\)

Consider a sample of calcium carbonate in the form of a cube measuring 2.005 in. on each edge. If the sample has a density of \(2.71 \mathrm{~g} / \mathrm{cm}^{3},\) how many oxygen atoms does it contain?

Balance the following equations: (a) \(\mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)\) (b) \(\mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HNO}_{3}(a q)\) (c) \(\mathrm{CH}_{4}(g)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CCl}_{4}(l)+\mathrm{HCl}(g)\) (d) \(\mathrm{Al}_{4} \mathrm{C}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{CH}_{4}(g)\) (e) \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}_{2}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (f) \(\mathrm{Fe}(\mathrm{OH})_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (g) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\) \(\mathrm{MgSO}_{4}(a q)+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)\)

(a) Define the terms limiting reactant and excess reactant. (b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant? (c) Why should you base your choice of which compound is the limiting reactant on its number of initial moles, not on its initial mass in grams?

A mixture containing \(\mathrm{KClO}_{3}, \mathrm{~K}_{2} \mathrm{CO}_{3}, \mathrm{KHCO}_{3},\) and \(\mathrm{KCl}\) was heated, producing \(\mathrm{CO}_{2}, \mathrm{O}_{2}\), and \(\mathrm{H}_{2} \mathrm{O}\) gases according to the following equations: $$ \begin{aligned} 2 \mathrm{KClO}_{3}(s) & \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g) \\\ 2 \mathrm{KHCO}_{3}(s) & \longrightarrow \mathrm{K}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(g)+2 \mathrm{CO}_{2}(g) \\ \mathrm{K}_{2} \mathrm{CO}_{3}(s) & \longrightarrow \mathrm{K}_{2} \mathrm{O}(s)+\mathrm{CO}_{2}(g) \end{aligned} $$ The KCl does not react under the conditions of the reaction. If \(100.0 \mathrm{~g}\) of the mixture produces \(1.80 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}, 13.20 \mathrm{~g}\) of \(\mathrm{CO}_{2}\), and \(4.00 \mathrm{~g}\) of \(\mathrm{O}_{2}\), what was the composition of the original mixture? (Assume complete decomposition of the mixture.)
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