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Chapter 3: Problem 22

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) \(\mathrm{NaClO}_{3}(s) \longrightarrow \mathrm{NaCl}(s)+\mathrm{O}_{2}(g)\) (b) $\mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NH}_{3}(g)$ (c) \(\mathrm{K}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{KCl}(s)\) (d) $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(l)$

Short Answer

Expert verified
(a) Balanced Equation: \( \mathrm{2 NaClO}_{3}(s) \longrightarrow \mathrm{2 NaCl}(s)+\frac{3}{2}\mathrm{O}_{2}(g) \), Decomposition Reaction (b) Balanced Equation: \( \mathrm{NH}_{4} \mathrm{OH}(a q) \longrightarrow \mathrm{H}_{2}\mathrm{O}(l)+\mathrm{NH}_{3}(g) \), Decomposition Reaction (c) Balanced Equation: \( \mathrm{2K}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{2KCl}(s) \), Combination Reaction (d) Balanced Equation: \( \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{3 O}_{2}(g) \longrightarrow \mathrm{2 CO}_{2}(\mathrm{~g})+\mathrm{3 H}_{2} \mathrm{O}(l) \), Combustion Reaction

Step by step solution

01

(a) Identify the type of reaction

In this reaction, a single compound, NaClO3, breaks down into two products, NaCl and O2. So, it is a decomposition reaction.
02

(a) Balance the equation

Balancing the decomposition reaction: NaClO3(s) -> NaCl(s) + O2(g) We can balance the oxygen atoms by multiplying the O2 by 1.5: \[ \mathrm{2 NaClO}_{3}(s) \longrightarrow \mathrm{2 NaCl}(s)+\frac{3}{2}\mathrm{O}_{2}(g) \]
03

(b) Identify the type of reaction

In this reaction, a single compound, NH4OH, breaks down into two products, H2O and NH3. So, it is a decomposition reaction.
04

(b) Balance the equation

Balancing the decomposition reaction: NH4OH(aq) -> H2O(l) + NH3(g) This equation is already balanced.
05

(c) Identify the type of reaction

In this reaction, two reactants (K and Cl2) are combining to form a single product (KCl). So, it is a combination reaction.
06

(c) Balance the equation

Balancing the combination reaction: K(s) + Cl2(g) -> KCl(s) We can balance the chlorine atoms by multiplying KCl by 2: \[ \mathrm{2K}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{2KCl}(s) \]
07

(d) Identify the type of reaction

In this reaction, a hydrocarbon, C2H5OH, reacts with O2, and the products are CO2 and H2O. This is a combustion reaction.
08

(d) Balance the equation

Balancing the combustion reaction: C2H5OH(l) + O2(g) -> CO2(g) + H2O(l) There are 2 carbon atoms, 6 hydrogen atoms, and 3 oxygen atoms on reactants side. There is 1 carbon atom, 2 hydrogen atoms, and 3 oxygen atoms on products side. So, we can balance by placing coefficients as follows: \[ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{3 O}_{2}(g) \longrightarrow \mathrm{2 CO}_{2}(\mathrm{~g})+\mathrm{3 H}_{2} \mathrm{O}(l) \]

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Most popular questions from this chapter

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of \(\mathrm{NH}_{3}\) to NO: $$ 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) $$ In a certain experiment, \(2.00 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) reacts with \(2.50 \mathrm{~g}\) of \(\mathrm{O}_{2}\). (a) Which is the limiting reactant? (b) How many grams of \(\mathrm{NO}\) and \(\mathrm{H}_{2} \mathrm{O}\) form? \((\mathbf{c})\) How many grams of the excess reactant remain after the limiting reactant is completely consumed? (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) $\mathrm{C}_{7} \mathrm{H}_{16}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)$ (b) $\mathrm{Li}_{3} \mathrm{~N}(s)+\mathrm{BN}(s) \longrightarrow \mathrm{Li}_{3} \mathrm{BN}_{2}(s)$ (c) $\mathrm{Zn}(\mathrm{OH})_{2}(s) \longrightarrow \mathrm{ZnO}(s)+\mathrm{H}_{2} \mathrm{O}(I)$ (d) $\mathrm{Ag}_{2} \mathrm{O}(s) \longrightarrow \mathrm{Ag}(s)+\mathrm{O}_{2}(g)$

The reaction between potassium superoxide, \(\mathrm{KO}_{2}\), and \(\mathrm{CO}_{2}\), $$ 4 \mathrm{KO}_{2}+2 \mathrm{CO}_{2} \longrightarrow 2 \mathrm{~K}_{2} \mathrm{CO}_{3}+3 \mathrm{O}_{2} $$ is used as a source of \(\mathrm{O}_{2}\) and absorber of \(\mathrm{CO}_{2}\) in selfcontained breathing equipment used by rescue workers. (a) How many moles of \(\mathrm{O}_{2}\) are produced when \(0.400 \mathrm{~mol}\) of \(\mathrm{KO}_{2}\) reacts in this fashion? (b) How many grams of \(\mathrm{KO}_{2}\) are needed to form \(7.50 \mathrm{~g}\) of \(\mathrm{O}_{2}\) ? (c) How many grams of \(\mathrm{CO}_{2}\) are used when \(7.50 \mathrm{~g}\) of \(\mathrm{O}_{2}\) are produced?

Determine the empirical and molecular formulas of each of the following substances: (a) Styrene, a compound used to make Styrofoam \(^{*}\) cups and insulation, contains \(92.3 \% \mathrm{C}\) and \(7.7 \% \mathrm{H}\) by mass and has a molar mass of \(104 \mathrm{~g} / \mathrm{mol}\). (b) Caffeine, a stimulant found in coffee, contains \(49.5 \% \mathrm{C}\), \(5.15 \% \mathrm{H}, 28.9 \% \mathrm{~N},\) and \(16.5 \% \mathrm{O}\) by mass and has a molar mass of \(195 \mathrm{~g} / \mathrm{mol}\) (c) Monosodium glutamate (MSG), a flavor enhancer in certain foods, contains \(35.51 \% \mathrm{C}, 4.77 \% \mathrm{H}, 37.85 \% \mathrm{O},\) $8.29 \% \mathrm{~N},\( and \)13.60 \% \mathrm{Na},\( and has a molar mass of \)169 \mathrm{~g} / \mathrm{mol} .$

Cinnamaldehyde is a compound that is responsible for the characteristic aroma of cinnamon. It contains \(81.79 \% \mathrm{C}\), \(6.10 \% \mathrm{H},\) and the remaining is oxygen. Its molar mass is \(132 \mathrm{~g} / \mathrm{mol} .\) Determine its molecular formula.
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