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Chapter 3: Problem 16

Write balanced chemical equations to correspond to each of the following descriptions: (a) When sulfur trioxide gas reacts with water, a solution of sulfuric acid forms. (b) Boron sulfide, \(\mathrm{B}_{2} \mathrm{~S}_{3}(s),\) reacts violently with water to form dissolved boric acid, $\mathrm{H}_{3} \mathrm{BO}_{3},$ and hydrogen sulfide gas. (c) Phosphine, \(\mathrm{PH}_{3}(g)\), combusts in oxygen gas to form water vapor and solid tetraphosphorus decaoxide. (d) When solid mercury(II) nitrate is heated, it decomposes to form solid mercury(II) oxide, gaseous nitrogen dioxide, and oxygen. (e) Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper(II) sulfate, sulfur dioxide gas, and water.

Short Answer

Expert verified
(a) \(SO_3 + H_2O \rightarrow H_2SO_4\) (b) \(B_2S_3 + 6H_2O \rightarrow 2H_3BO_3 + 3H_2S\) (c) \(4PH_3 + 8O_2 \rightarrow 6H_2O + P_4O_{10}\) (d) \(2Hg(NO_3)_2 \rightarrow 2HgO + 4NO_2 + O_2\) (e) \(Cu + H_2SO_4 \rightarrow CuSO_4 + SO_2 + H_2O\)

Step by step solution

01

Write the unbalanced equation

The chemical formula for sulfur trioxide is SO₃, and for water it is H₂O. They react to form sulfuric acid (H₂SO₄). The unbalanced equation is: SO₃ + H₂O → H₂SO₄
02

Balance the equation

The equation is already balanced: SO₃ + H₂O → H₂SO₄ (b) Boron sulfide reacts violently with water to form boric acid and hydrogen sulfide gas.
03

Write the unbalanced equation

The chemical formula for boron sulfide is B₂S₃, and it reacts with water (H₂O) to form boric acid (H₃BO₃) and hydrogen sulfide gas (H₂S). The unbalanced equation is: B₂S₃ + H₂O → H₃BO₃ + H₂S
04

Balance the equation

Balancing the equation gives us: B₂S₃ + 6H₂O → 2H₃BO₃ + 3H₂S (c) Phosphine combusts in oxygen gas to form water vapor and solid tetraphosphorus decaoxide.
05

Write the unbalanced equation

Phosphine (PH₃) combusts in oxygen (O₂) to form water vapor (H₂O) and solid tetraphosphorus decaoxide (P₄O₁₀). The unbalanced equation is: PH₃ + O₂ → H₂O + P₄O₁₀
06

Balance the equation

Balancing the equation gives us: 4PH₃ + 8O₂ → 6H₂O + P₄O₁₀ (d) Solid mercury(II) nitrate decomposes to form solid mercury(II) oxide, nitrogen dioxide, and oxygen.
07

Write the unbalanced equation

When solid mercury(II) nitrate (Hg(NO₃)₂) is heated, it decomposes to form solid mercury(II) oxide (HgO), nitrogen dioxide (NO₂), and oxygen (O₂). The unbalanced equation is: Hg(NO₃)₂ → HgO + NO₂ + O₂
08

Balance the equation

Balancing the equation gives us: 2Hg(NO₃)₂ → 2HgO + 4NO₂ + O₂ (e) Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper(II) sulfate, sulfur dioxide gas, and water.
09

Write the unbalanced equation

Copper (Cu) reacts with hot concentrated sulfuric acid (H₂SO₄) to form aqueous copper(II) sulfate (CuSO₄), sulfur dioxide gas (SO₂), and water (H₂O). The unbalanced equation is: Cu + H₂SO₄ → CuSO₄ + SO₂ + H₂O
10

Balance the equation

Balancing the equation gives us: Cu + H₂SO₄ → CuSO₄ + SO₂ + H₂O

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Most popular questions from this chapter

Calculate the percentage by mass of the indicated element in the following compounds: (a) hydrogen in methane, \(\mathrm{CH}_{4}\), the major hydrocarbon in natural gas; \((\mathbf{b})\) oxygen in vitamin $\mathrm{E}, \mathrm{C}_{29} \mathrm{H}_{50} \mathrm{O}_{2} ;$ (c) sulphur in magnesium sulphate, \(\mathrm{MgSO}_{4}\), a substance used as a drying agent; \((\mathbf{d})\) nitrogen in epinephrine, \(\mathrm{C}_{9} \mathrm{H}_{13} \mathrm{NO}_{3},\) also known as adrenalin, a hormone that is important for the fightor-flight response; (e) oxygen in the insect pheromone sulcatol, $\mathrm{C}_{8} \mathrm{H}_{16} \mathrm{O} ;\( (f) carbon in sucrose, \)\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11},$ the compound that is responsible for the sweet taste of table sugar.

Several brands of antacids use \(\mathrm{Al}(\mathrm{OH})_{3}\) to react with stomach acid, which contains primarily HCl: $$ \mathrm{Al}(\mathrm{OH})_{3}(s)+\mathrm{HCl}(a q) \longrightarrow \mathrm{AlCl}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ (a) Balance this equation. (b) Calculate the number of grams of HCl that can react with $0.500 \mathrm{~g}\( of \)\mathrm{Al}(\mathrm{OH})_{3}$ (c) Calculate the number of grams of \(\mathrm{AlCl}_{3}\) and the number of grams of \(\mathrm{H}_{2} \mathrm{O}\) formed when \(0.500 \mathrm{~g}\) of \(\mathrm{Al}(\mathrm{OH})_{3}\) reacts. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

Determine the formula weights of each of the following compounds: (a) Butyric acid, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{COOH},\) which is responsible for the rotten smell of spoiled food; (b) sodium perborate, \(\mathrm{NaBO}_{3}\), a substance used as bleach; (c) calcium carbonate, \(\mathrm{CaCO}_{3},\) a substance found in marble. (c) $\mathrm{CF}_{2} \mathrm{Cl}_{2},\( a refrigerant known as Freon; \)(\mathbf{d}) \mathrm{NaHCO}_{3},$ known as baking soda and used in bread and pastry baking; \((\mathbf{e})\) iron pyrite, \(\mathrm{FeS}_{2}\) which has a golden appearance and is known as "Fool's Gold."

Very small semiconductor crystals, composed of approximately 1000 to 10,000 atoms, are called quantum dots. Quantum dots made of the semiconductor CdSe are now being used in electronic reader and tablet displays because they emit light efficiently and in multiple colors, depending on dot size. The density of CdSe is \(5.82 \mathrm{~g} / \mathrm{cm}^{3}\) (a) What is the mass of one \(2.5-\mathrm{nm}\) CdSe quantum dot? (b) CdSe quantum dots that are \(2.5 \mathrm{nm}\) in diameter emit blue light upon stimulation. Assuming that the dot is a perfect sphere and that the empty space in the dot can be neglected, calculate how many Cd atoms are in one quantum dot of this size. (c) What is the mass of one \(6.5-\mathrm{nm}\) CdSe quantum dot? (d) CdSe quantum dots that are \(6.5 \mathrm{nm}\) in diameter emit red light upon stimulation. Assuming that the dot is a perfect sphere, calculate how many Cd atoms are in one quantum dot of this size. (e) If you wanted to make one \(6.5-\mathrm{nm}\) dot from multiple \(2.5-\mathrm{nm}\) dots, how many \(2.5-\mathrm{nm}\) dots would you need, and how many CdSe formula units would be left over, if any?

Determine the empirical formulas of the compounds with the following compositions by mass: (a) \(74.0 \% \mathrm{C}, 8.7 \% \mathrm{H},\) and \(17.3 \% \mathrm{~N}\) (b) \(57.5 \% \mathrm{Na}, 40.0 \% \mathrm{O},\) and \(2.5 \% \mathrm{H}\) (c) \(41.1 \% \mathrm{~N}, 11.8 \% \mathrm{H},\) and the remainder \(\mathrm{S}\)
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