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Chapter 3: Problem 98

Give the balanced equation for each of the following. a. The combustion of ethanol $\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)$ forms carbon dioxide and water vapor. A combustion reaction refers to a reaction of a substance with oxygen gas. b. Aqueous solutions of lead(Il) nitrate and sodium phosphate are mixed, resulting in the precipitate formation of lead(II) phosphate with aqueous sodium nitrate as the other product. c. Solid zinc reacts with aqueous HCl to form aqueous zinc chloride and hydrogen gas. d. Aqueous strontium hydroxide reacts with aqueous hydrobromic acid to produce water and aqueous strontium bromide.

Short Answer

Expert verified
a. \[ C_{2}H_{5}OH + \frac{3}{2}O_{2} \rightarrow 2CO_{2} + 3H_{2}O \] b. \[ 3Pb(NO_{3})_{2} + 2Na_{3}PO_{4} \rightarrow Pb_{3}(PO_{4})_{2} + 6NaNO_{3} \] c. \[ Zn + 2HCl \rightarrow ZnCl_{2} + H_{2} \] d. \[ Sr(OH)_{2} + 2HBr \rightarrow 2H_{2}O + SrBr_{2} \]

Step by step solution

01

a. Combustion of Ethanol

1. Write the unbalanced equation: Ethanol (C2H5OH) reacts with oxygen (O2) to form carbon dioxide (CO2) and water (H2O). \[ C_{2}H_{5}OH + O_{2} \rightarrow CO_{2} + H_{2}O \] 2. Balance the equation: To balance this equation, we need to ensure that the number of each type of atom on the reactants side is equal to the number of each type of atom on the products side. \[ C_{2}H_{5}OH + \frac{3}{2}O_{2} \rightarrow 2CO_{2} + 3H_{2}O \] The balanced equation for the combustion of ethanol is: \[ C_{2}H_{5}OH + \frac{3}{2}O_{2} \rightarrow 2CO_{2} + 3H_{2}O \]
02

b. Precipitate formation between lead(II) nitrate and sodium phosphate

1. Write the unbalanced equation: Lead(II) nitrate (Pb(NO3)2) reacts with sodium phosphate (Na3PO4) to form lead(II) phosphate (Pb3(PO4)2) and sodium nitrate (NaNO3). \[ Pb(NO_{3})_{2} + Na_{3}PO_{4} \rightarrow Pb_{3}(PO_{4})_{2} + NaNO_{3} \] 2. Balance the equation: To balance the equation, ensure that the number of each type of atom on the reactants side is equal to the number of each type of atom on the products side. \[ 3Pb(NO_{3})_{2} + 2Na_{3}PO_{4} \rightarrow Pb_{3}(PO_{4})_{2} + 6NaNO_{3} \] The balanced equation for the precipitate formation between lead(II) nitrate and sodium phosphate is: \[ 3Pb(NO_{3})_{2} + 2Na_{3}PO_{4} \rightarrow Pb_{3}(PO_{4})_{2} + 6NaNO_{3} \]
03

c. Reaction of solid zinc with aqueous HCl

1. Write the unbalanced equation: Solid zinc (Zn) reacts with aqueous HCl (HCl) to form aqueous zinc chloride (ZnCl2) and hydrogen gas (H2). \[ Zn + HCl \rightarrow ZnCl_{2} + H_{2} \] 2. Balance the equation: To balance the equation, ensure that the number of each type of atom on the reactants side is equal to the number of each type of atom on the products side. \[ Zn + 2HCl \rightarrow ZnCl_{2} + H_{2} \] The balanced equation for the reaction of solid zinc with aqueous HCl is: \[ Zn + 2HCl \rightarrow ZnCl_{2} + H_{2} \]
04

d. Reaction of aqueous strontium hydroxide with aqueous hydrobromic acid

1. Write the unbalanced equation: Aqueous strontium hydroxide (Sr(OH)2) reacts with aqueous hydrobromic acid (HBr) to form water (H2O) and aqueous strontium bromide (SrBr2). \[ Sr(OH)_{2} + HBr \rightarrow H_{2}O + SrBr_{2} \] 2. Balance the equation: To balance the equation, ensure that the number of each type of atom on the reactants side is equal to the number of each type of atom on the products side. \[ Sr(OH)_{2} + 2HBr \rightarrow 2H_{2}O + SrBr_{2} \] The balanced equation for the reaction of aqueous strontium hydroxide with aqueous hydrobromic acid is: \[ Sr(OH)_{2} + 2HBr \rightarrow 2H_{2}O + SrBr_{2} \]

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Most popular questions from this chapter

The space shuttle environmental control system handled excess \(\mathrm{CO}_{2}\) (which the astronauts breathe out; it is 4.0\(\%\) by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li \(_{2} \mathrm{CO}_{3},\) and water. If there were seven astronauts on board the shuttle, and each exhales \(20 .\) L of air per minute, how long could clean air be generated if there were \(25,000\) g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 \(\mathrm{g} / \mathrm{mL}\) .

a. Write the balanced equation for the combustion of isooctane \(\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)\) to produce water vapor and carbon dioxide gas. b. Assuming gasoline is \(100 . \%\) isooctane, with a density of 0.692 \(\mathrm{g} / \mathrm{mL}\) , what is the theoretical yield of carbon dioxide produced by the combustion of \(1.2 \times 10^{10}\) gal of gasoline (the approximate annual consumption of gasoline in the United States)?

Phosphorus can be prepared from calcium phosphate by the following reaction: $$ 2 \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+6 \mathrm{SiO}_{2}(s)+10 \mathrm{C}(s) \longrightarrow $$ $$ 6 \mathrm{CaSiO}_{3}(s)+\mathrm{P}_{4}(s)+10 \mathrm{CO}(g) $$ Phosphorite is a mineral that contains \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) plus other non-phosphorus-containing compounds. What is the maximum amount of \(\mathrm{P}_{4}\) that can be produced from 1.0 \(\mathrm{kg}\) of phosphorite if the phorphorite sample is 75$\% \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}$ by mass? Assume an excess of the other reactants.

Iron oxide ores, commonly a mixture of FeO and $\mathrm{Fe}_{2} \mathrm{O}_{3},\( are given the general formula \)\mathrm{Fe}_{3} \mathrm{O}_{4}$ . They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes: $$ \begin{array}{c}{\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{O}(g)} \\\ {\mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g)}\end{array} $$

Aluminum reacts with bromine, producing aluminum bromide: $$ 2 \mathrm{Al}(s)+3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{AlBr}_{3}(s) $$ In a certain experiment, 20.0 \(\mathrm{mL}\) of bromine (density \(=\) 3.10 \(\mathrm{g} / \mathrm{mL}\) ) was reacted with excess aluminum to yield 50.3 \(\mathrm{g}\) of aluminum bromide. What is the percent yield for this experiment?
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