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Chapter 3: Problem 90

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(II) 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 \(\mathrm{HCl}\) 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. \[2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} + 3 \mathrm{O}_{2} \to 4 \mathrm{CO}_{2} + 6 \mathrm{H}_{2} \mathrm{O}\] b. \[2 \mathrm{Pb(NO}_{3}\mathrm{)_{2}\mathrm{(aq)} + 3 \mathrm{Na}_{3} \mathrm{PO}_{4}\mathrm{(aq)} \to \mathrm{Pb}_{3}(\mathrm{PO}_{4})_{2}\mathrm{(s)} + 6 \mathrm{NaNO}_{3}\mathrm{(aq)}\] c. \[\mathrm{Zn(s)} + 2 \mathrm{HCl(aq)} \to \mathrm{ZnCl}_{2}\mathrm{(aq)} + \mathrm{H}_{2}\mathrm{(g)}\] d. \[\mathrm{Sr(OH)}_{2}\mathrm{(aq)} + 2 \mathrm{HBr(aq)} \to 2 \mathrm{H}_{2}\mathrm{O} + \mathrm{SrBr}_{2}\mathrm{(aq)}\]

Step by step solution

01

Identify the reactants and products

In a combustion reaction, the reactant is a substance that reacts with oxygen gas. In this case, the reactant is ethanol, which has the chemical formula \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\). The products of combustion are carbon dioxide (\(\mathrm{CO}_{2}\)) and water vapor (\(\mathrm{H}_{2} \mathrm{O}\)).
02

Write the unbalanced chemical equation

Using the reactants and products, the unbalanced equation can be written as: \[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} + \mathrm{O}_{2} \to \mathrm{CO}_{2} + \mathrm{H}_{2} \mathrm{O}\]
03

Balance the chemical equation

To balance the equation, we will first count the number of atoms for each element on both sides of the equation: - Carbon: 2 atoms in ethanol - Hydrogen: 6 atoms in ethanol - Oxygen: 3 atoms in ethanol and oxygen gas Now we will adjust the coefficients to balance the equation: \[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} + \dfrac{3}{2} \mathrm{O}_{2} \to 2 \mathrm{CO}_{2} + 3 \mathrm{H}_{2} \mathrm{O}\] However, it is generally preferable to have whole-number coefficients, so we will multiply each coefficient by 2 to achieve this: \[2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} + 3 \mathrm{O}_{2} \to 4 \mathrm{CO}_{2} + 6 \mathrm{H}_{2} \mathrm{O}\] b. Mixing of aqueous lead(II) nitrate and sodium phosphate
04

Identify the reactants and products

The reactants are aqueous solutions of lead(II) nitrate and sodium phosphate. Lead(II) nitrate has the chemical formula \(\mathrm{Pb(NO}_{3}\mathrm{)_{2}\), and sodium phosphate has the chemical formula \(\mathrm{Na}_{3} \mathrm{PO}_{4}\). The products are solid lead(II) phosphate (\(\mathrm{Pb}_{3}(\mathrm{PO}_{4})_{2}\)) and aqueous sodium nitrate (\(\mathrm{NaNO}_{3}\)).
05

Write the unbalanced chemical equation

Plugging in the reactants and products, we have: \[\mathrm{Pb(NO}_{3}\mathrm{)_{2}\mathrm{(aq)} + \mathrm{Na}_{3} \mathrm{PO}_{4}\mathrm{(aq)} \to \mathrm{Pb}_{3}(\mathrm{PO}_{4})_{2}\mathrm{(s)} + \mathrm{NaNO}_{3}\mathrm{(aq)}\]
06

Balance the chemical equation

Adjust the coefficients to balance the atoms of each element: \[2 \mathrm{Pb(NO}_{3}\mathrm{)_{2}\mathrm{(aq)} + 3 \mathrm{Na}_{3} \mathrm{PO}_{4}\mathrm{(aq)} \to \mathrm{Pb}_{3}(\mathrm{PO}_{4})_{2}\mathrm{(s)} + 6 \mathrm{NaNO}_{3}\mathrm{(aq)}\] c. Reaction of solid zinc with aqueous \(\mathrm{HCl}\)
07

Identify the reactants and products

The reactants are solid zinc (\(\mathrm{Zn}\)) and aqueous hydrochloric acid (\(\mathrm{HCl}\)). The products are aqueous zinc chloride (\(\mathrm{ZnCl}_{2}\)) and hydrogen gas (\(\mathrm{H}_{2}\)).
08

Write the unbalanced chemical equation

Combine the reactants and products: \[\mathrm{Zn(s)} + \mathrm{HCl(aq)} \to \mathrm{ZnCl}_{2}\mathrm{(aq)} + \mathrm{H}_{2}\mathrm{(g)}\]
09

Balance the chemical equation

Adjust the coefficients: \[\mathrm{Zn(s)} + 2 \mathrm{HCl(aq)} \to \mathrm{ZnCl}_{2}\mathrm{(aq)} + \mathrm{H}_{2}\mathrm{(g)}\] d. Reaction of aqueous strontium hydroxide with aqueous hydrobromic acid
10

Identify the reactants and products

The reactants are aqueous strontium hydroxide (\(\mathrm{Sr(OH)}_{2}\)) and aqueous hydrobromic acid (\(\mathrm{HBr}\)). The products are water (\(\mathrm{H}_{2}\mathrm{O}\)) and aqueous strontium bromide (\(\mathrm{SrBr}_{2}\)).
11

Write the unbalanced chemical equation

Combine the reactants and products: \[\mathrm{Sr(OH)}_{2}\mathrm{(aq)} + \mathrm{HBr(aq)} \to \mathrm{H}_{2}\mathrm{O} + \mathrm{SrBr}_{2}\mathrm{(aq)}\]
12

Balance the chemical equation

Adjust the coefficients: \[\mathrm{Sr(OH)}_{2}\mathrm{(aq)} + 2 \mathrm{HBr(aq)} \to 2 \mathrm{H}_{2}\mathrm{O} + \mathrm{SrBr}_{2}\mathrm{(aq)}\]

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Most popular questions from this chapter

Acrylonitrile \(\left(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}\right)\) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction. \(2 \mathrm{C}_{3} \mathrm{H}_{6}(g)+2 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\) If \(15.0 \mathrm{~g} \mathrm{C}_{3} \mathrm{H}_{6}, 10.0 \mathrm{~g} \mathrm{O}_{2}\), and \(5.00 \mathrm{~g} \mathrm{NH}_{3}\) are reacted, what mass of acrylonitrile can be produced, assuming \(100 \%\) yield?

Consider the following unbalanced reaction: $$ \mathrm{P}_{4}(s)+\mathrm{F}_{2}(g) \longrightarrow \mathrm{PF}_{3}(g) $$ What mass of \(\mathrm{F}_{2}\) is needed to produce \(120 . \mathrm{g}\) of \(\mathrm{PF}_{3}\) if the reaction has a \(78.1 \%\) yield?

An ionic compound \(\mathrm{MX}_{3}\) is prepared according to the following unbalanced chemical equation. $$ \mathrm{M}+\mathrm{X}_{2} \longrightarrow \mathrm{MX}_{3} $$ A \(0.105-g\) sample of \(X_{2}\) contains \(8.92 \times 10^{20}\) molecules. The compound \(\mathrm{MX}_{3}\) consists of \(54.47 \% \mathrm{X}\) by mass. What are the identities of \(\mathrm{M}\) and \(\mathrm{X}\), and what is the correct name for \(\mathrm{MX}_{3}\) ? Starting with \(1.00 \mathrm{~g}\) each of \(\mathrm{M}\) and \(\mathrm{X}_{2}\), what mass of \(\mathrm{MX}_{3}\) can be prepared?

When aluminum metal is heated with an element from Group \(6 \mathrm{~A}\) of the periodic table, an ionic compound forms. When the experiment is performed with an unknown Group \(6 \mathrm{~A}\) element, the product is \(18.56 \%\) Al by mass. What is the formula of the compound?

A \(2.077-g\) sample of an element, which has an atomic mass between 40 and 55 , reacts with oxygen to form \(3.708 \mathrm{~g}\) of an oxide. Determine the formula of the oxide (and identify the element).
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