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Chapter 3: Problem 20

Write a balanced chemical equation for the reaction that occurs when (a) titanium metal reacts with \(\mathrm{O}_{2}(g) ;(\mathbf{b})\) silver(I) oxide decomposes into silver metal and oxygen gas when heated; (c) propanol, \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(l)\) burns in air; \((\mathbf{d})\) methyl tert-butyl ether, \(\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{O}(l),\) burns in air.

Short Answer

Expert verified
The balanced equations for the given reactions are: a) \(Ti(s) + O_{2}(g) \rightarrow TiO_{2}(s)\) b) \(2 Ag_{2}O(s) \rightarrow 4Ag(s) + O_{2}(g)\) c) \(2 C_{3}H_{7}OH(l) + 9 O_{2}(g) \rightarrow 6 CO_{2}(g) + 8 H_{2}O(l)\) d) \(C_{5}H_{12}O(l) + 8 O_{2}(g) \rightarrow 5 CO_{2}(g) + 6 H_{2}O(l)\)

Step by step solution

01

Write the basic unbalanced equation

In this reaction, Titanium (Ti) reacts with oxygen gas (O2) to form Titanium dioxide (TiO2). The unbalanced equation is: Ti(s) + O2(g) -> TiO2(s)
02

Balance the equation

As the equation is already balanced with coefficients 1:1:1, the final balanced equation is: Ti(s) + O2(g) -> TiO2(s) #b) Silver(I) oxide decomposes into silver metal and oxygen gas when heated#
03

Write the basic unbalanced equation

In this reaction, Silver(I) oxide (Ag2O) decomposes into silver metal (Ag) and oxygen gas (O2) when heated. The unbalanced equation is: Ag2O(s) -> Ag(s) + O2(g)
04

Balance the equation

To balance the equation, introduce the coefficients 2 for Ag and 1/2 for O2: Ag2O(s) -> 2Ag(s) + 1/2 O2(g)
05

Remove fractional coefficients

To remove the fractional coefficients, multiply all coefficients by 2: 2 Ag2O(s) -> 4Ag(s) + O2(g) #c) Propanol C3H7OH(l) burns in air#
06

Write the basic unbalanced equation

In this reaction, Propanol (C3H7OH) reacts with oxygen gas (O2) to form carbon dioxide (CO2) and water (H2O). The unbalanced equation is: C3H7OH(l) + O2(g) -> CO2(g) + H2O(l)
07

Balance the equation

To balance the equation, introduce coefficients for each species: C3H7OH(l) + 4.5 O2(g) -> 3 CO2(g) + 4 H2O(l)
08

Remove fractional coefficients

To remove the fractional coefficients, multiply all coefficients by 2: 2 C3H7OH(l) + 9 O2(g) -> 6 CO2(g) + 8 H2O(l) #d) Methyl tert-butyl ether C5H12O(l) burns in air#
09

Write the basic unbalanced equation

In this reaction, Methyl tert-butyl ether (C5H12O) reacts with oxygen gas (O2) to form carbon dioxide (CO2) and water (H2O). The unbalanced equation is: C5H12O(l) + O2(g) -> CO2(g) + H2O(l)
10

Balance the equation

To balance the equation, introduce coefficients for each species: C5H12O(l) + 8 O2(g) -> 5 CO2(g) + 6 H2O(l) The balanced equations for the given reactions are: a) Ti(s) + O2(g) -> TiO2(s) b) 2 Ag2O(s) -> 4Ag(s) + O2(g) c) 2 C3H7OH(l) + 9 O2(g) -> 6 CO2(g) + 8 H2O(l) d) C5H12O(l) + 8 O2(g) -> 5 CO2(g) + 6 H2O(l)

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Most popular questions from this chapter

Write balanced chemical equations for \((\mathbf{a})\) the complete combustion of acetone \(\left(\mathrm{CH}_{3} \mathrm{COCH}_{3}\right),\) a common organic solvent; (b) the decomposition of solid mercury (I) carbonate into carbon dioxide gas, mercury, and solid mercury oxide; (c) the combination reaction between sulphur dioxide gas and liquid water to produce sulfurous acid.

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.

Write a balanced chemical equation for the reaction that occurs when (a) \(\mathrm{Mg}(s)\) reacts with \(\mathrm{Cl}_{2}(g) ;(\mathbf{b})\) barium carbonate decomposes into barium oxide and carbon dioxide gas when heated; \((\mathbf{c})\) the hydrocarbon styrene, \(\mathrm{C}_{8} \mathrm{H}_{8}(l),\) is combusted in air; \((\mathbf{d})\) dimethylether, $\mathrm{CH}_{3} \mathrm{OCH}_{3}(g),$ is combusted in air.

What is the mass, in kilograms, of an Avogadro's number of people, if the average mass of a person is \(160 \mathrm{lb}\) ? How does this compare with the mass of Earth, \(5.98 \times 10^{24} \mathrm{~kg}\) ?

Hydrofluoric acid, HF \((a q)\), cannot be stored in glass bottles because compounds called silicates in the glass are attacked by the $\mathrm{HF}(a q)\(. Sodium silicate \)\left(\mathrm{Na}_{2} \mathrm{SiO}_{3}\right),$ for example, reacts as follows: $$ \mathrm{Na}_{2} \mathrm{SiO}_{3}(s)+8 \mathrm{HF}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{SiF}_{6}(a q)+2 \mathrm{NaF}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l) $$ (a) How many moles of HF are needed to react with 0.300 mol of \(\mathrm{Na}_{2} \mathrm{SiO}_{3} ?\) (b) How many grams of NaF form when \(0.500 \mathrm{~mol}\) of HF reacts with excess \(\mathrm{Na}_{2} \mathrm{SiO}_{3} ?\) (c) How many grams of \(\mathrm{Na}_{2} \mathrm{SiO}_{3}\) can react with $0.800 \mathrm{~g}$ of HF?
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