/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 20 Balance the following equations,... [FREE SOLUTION] | 91影视

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Chapter 3: Problem 20

Balance the following equations, and indicate whether they are combination, decomposition, or combustion reactions: (a) \(\mathrm{C}_{3} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (b) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (c) \(\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (d) \(\mathrm{N}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{NH}_{3}(g)\) (e) \(\mathrm{K}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{KOH}(a q)\)

Short Answer

Expert verified
(a) Balanced equation: \(C_3H_6(g) + \frac{9}{2}O_2(g) \rightarrow 3CO_2(g) + 3H_2O(g)\) | Combustion (b) Balanced equation: \(NH_4NO_3(s) \rightarrow N_2O(g) + 2H_2O(g)\) | Decomposition (c) Balanced equation: \(C_5H_6O(l) + \frac{15}{2}O_2(g) \rightarrow 5CO_2(g) + 3H_2O(g)\) | Combustion (d) Balanced equation: \(N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)\) | Combination (e) Balanced equation: \(K_2O(s) + H_2O(l) \rightarrow 2KOH(aq)\) | Combination

Step by step solution

01

Balancing the equation

To balance this chemical equation, we need to ensure that the number of atoms for each element on both sides of the equation are equal. Balanced equation: \(\mathrm{C}_{3} \mathrm{H}_{6}(g) +\dfrac{9}{2}\mathrm{O}_{2}(g) \longrightarrow 3\mathrm{CO}_{2}(g) +3\mathrm{H}_{2} \mathrm{O}(g)\)
02

Identifying the reaction type

A combustion reaction is characterized by reactants (usually a hydrocarbon) and oxygen, forming carbon dioxide and water. This equation fits that pattern making it a combustion reaction. (b) \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)
03

Balancing the equation

Balanced equation: \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) \longrightarrow \mathrm{N}_{2} \mathrm{O}(g) +2\mathrm{H}_{2} \mathrm{O}(g)\)
04

Identifying the reaction type

A decomposition reaction typically involves a single reactant being broken down into multiple products. This equation meets that requirement meaning it is a decomposition reaction. (c) \(\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)
05

Balancing the equation

Balanced equation: \(\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}(l) + \dfrac{15}{2}\mathrm{O}_{2}(g) \longrightarrow 5\mathrm{CO}_{2}(g) + 3\mathrm{H}_{2} \mathrm{O}(g)\)
06

Identifying the reaction type

This reaction also fits the pattern of a combustion reaction. (d) \(\mathrm{N}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{NH}_{3}(g)\)
07

Balancing the equation

Balanced equation: \(\mathrm{N}_{2}(g)+3\mathrm{H}_{2}(g) \longrightarrow 2\mathrm{NH}_{3}(g)\)
08

Identifying the reaction type

A combination reaction includes two or more reactants combining to form a single product. This reaction matches the pattern making it a combination reaction. (e) \(\mathrm{K}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{KOH}(a q)\)
09

Balancing the equation

Balanced equation: \(\mathrm{K}_{2} \mathrm{O}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2\mathrm{KOH}(a q)\)
10

Identifying the reaction type

This reaction also follows the pattern of a combination reaction, where the two reactants combine to form a single product.

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Most popular questions from this chapter

Vanillin, the dominant flavoring in vanilla, contains \(\mathrm{C}\), \(\mathrm{H}\), and \(\mathrm{O}\). When \(1.05 \mathrm{~g}\) of this substance is completely combusted, \(2.43 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) and \(0.50 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) are produced. What is the empirical formula of vanillin?

Sodium hydroxide reacts with carbon dioxide as follows: $$ 2 \mathrm{NaOH}(s)+\mathrm{CO}_{2}(g) \longrightarrow \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) $$ Which reagent is the limiting reactant when \(1.85 \mathrm{~mol}\) \(\mathrm{NaOH}\) and \(1.00 \mathrm{~mol} \mathrm{CO}_{2}\) are allowed to react? How many moles of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) can be produced? How many moles of the excess reactant remain after the completion of the reaction?

An element \(X\) forms an iodide \(\left(\mathrm{XI}_{3}\right)\) and a chloride \(\left(\mathrm{XCl}_{3}\right) .\) The iodide is quantitatively converted to the chloride when it is heated in a stream of chlorine: $$ 2 \mathrm{XI}_{3}+3 \mathrm{Cl}_{2} \longrightarrow 2 \mathrm{XCl}_{3}+3 \mathrm{I}_{2} $$ If \(0.5000 \mathrm{~g}\) of \(\mathrm{XI}_{3}\) is treated, \(0.2360 \mathrm{~g}\) of \(\mathrm{XCl}_{3}\) is obtained. (a) Calculate the atomic weight of the element \(\mathrm{X}\) (b) Identify the element \(\bar{X}\).

Calculate the percentage by mass of oxygen in the following compounds: (a) morphine, \(\mathrm{C}_{17} \mathrm{H}_{19} \mathrm{NO}_{3}\); (b) codeine, \(\mathrm{C}_{18} \mathrm{H}_{21} \mathrm{NO}_{3} ;\) (c) cocaine, \(\mathrm{C}_{17} \mathrm{H}_{21} \mathrm{NO}_{4}\) (d) tetracycline, \(\mathrm{C}_{22} \mathrm{H}_{24} \mathrm{~N}_{2} \mathrm{O}_{8} ;\) (e) digitoxin, \(\mathrm{C}_{4} \mathrm{H}_{64} \mathrm{O}_{13} ;\) (f) vancomycin, \(\mathrm{C}_{66} \mathrm{H}_{75} \mathrm{Cl}_{2} \mathrm{~N}_{g} \mathrm{O}_{24}\)

Without doing any detailed calculations (but using a periodic table to give atomic weights), rank the following samples in order of increasing number of atoms: \(0.50 \mathrm{~mol} \mathrm{H}_{2} \mathrm{O}, 23 \mathrm{~g} \mathrm{Na}, 6.0 \times 10^{23} \mathrm{~N}_{2}\) molecules.
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