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Chapter 3: Problem 17

Write a balanced chemical equation for the reaction that occurs when (a) \(\mathrm{Mg}(s)\) reacts with \(\mathrm{Cl}_{2}(g) ;\) (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; (d) dimethylether, \(\mathrm{CH}_{3} \mathrm{OCH}_{3}(g)\), is combusted in air.

Short Answer

Expert verified
a) \( \mathrm{Mg}(s) + \mathrm{Cl}_{2}(g) \rightarrow \mathrm{MgCl}_{2}(s) \) b) \( \mathrm{BaCO}_{3}(s) \xrightarrow{\Delta} \mathrm{BaO}(s) + \mathrm{CO}_{2}(g) \) c) \( \mathrm{C}_{8} \mathrm{H}_{8}(l) + 6 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{CO}_{2}(g) + 4 \mathrm{H}_{2}\mathrm{O}(l) \) d) \( 2 \mathrm{CH}_{3} \mathrm{OCH}_{3}(g) + 3 \mathrm{O}_{2}(g) \rightarrow 3 \mathrm{CO}_{2}(g) + 4 \mathrm{H}_{2}\mathrm{O}(l) \)

Step by step solution

01

a) Magnesium reacts with chlorine gas

The reaction between magnesium (Mg) and chlorine gas (Cl2) will produce magnesium chloride (MgCl2). The balanced chemical equation is: \[ \mathrm{Mg}(s) + \mathrm{Cl}_{2}(g) \rightarrow \mathrm{MgCl}_{2}(s) \]
02

b) Barium carbonate decomposes into barium oxide and carbon dioxide gas when heated

Upon heating, barium carbonate (BaCO3) decomposes into barium oxide (BaO) and carbon dioxide gas (CO2). The balanced chemical equation for this reaction is: \[ \mathrm{BaCO}_{3}(s) \xrightarrow{\Delta} \mathrm{BaO}(s) + \mathrm{CO}_{2}(g) \]
03

c) Combustion of styrene (C8H8) in air

The combustion of styrene (C8H8) in the presence of oxygen (O2) will produce carbon dioxide (CO2) and water (H2O). The balanced chemical equation for this reaction is: \[ \mathrm{C}_{8} \mathrm{H}_{8}(l) + 6 \mathrm{O}_{2}(g) \rightarrow 8 \mathrm{CO}_{2}(g) + 4 \mathrm{H}_{2}\mathrm{O}(l) \]
04

d) Combustion of dimethylether (CH3OCH3) in air

The combustion of dimethylether (CH3OCH3) in the presence of oxygen (O2) will produce carbon dioxide (CO2) and water (H2O). The balanced chemical equation for this reaction is: \[ 2 \mathrm{CH}_{3} \mathrm{OCH}_{3}(g) + 3 \mathrm{O}_{2}(g) \rightarrow 3 \mathrm{CO}_{2}(g) + 4 \mathrm{H}_{2}\mathrm{O}(l) \]

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Most popular questions from this chapter

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: \(9.0 \times 10^{23}\) molecules of \(\mathrm{H}_{2} \mathrm{O}_{2}, 2.0 \mathrm{~mol} \mathrm{CH}_{4}, 16 \mathrm{~g} \mathrm{O}_{2}\)

Copper is an excellent electrical conductor widely used in making electric circuits. In producing a printed circuit board for the electronics industry, a layer of copper is laminated on a plastic board. A circuit pattern is then printed on the board using a chemically resistant polymer. The board is then exposed to a chemical bath that reacts with the exposed copper, leaving the desired copper circuit, which has been protected by the overlaying polymer. Finally, a solvent removes the polymer. One reaction used to remove the exposed copper from the circuit board is $$ \begin{aligned} \mathrm{Cu}(s)+\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}(a q)+4 \mathrm{NH}_{3}(a q) & \longrightarrow \\ & 2 \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}(a q) \end{aligned} $$ A plant needs to produce 5000 circuit boards, each with a surface area measuring 2.0 in. \(\times 3.0\) in. The boards are covered with a \(0.65-\mathrm{mm}\) layer of copper. In subsequent processing, \(85 \%\) of the copper is removed. Copper has a density of \(8.96 \mathrm{~g} / \mathrm{cm}^{3} .\) Calculate the masses of \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\) and \(\mathrm{NH}_{3}\) needed to produce the circuit boards, assuming that the reaction used gives a \(97 \%\) yield.

An iron ore sample contains \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) together with other substances. Reaction of the ore with CO produces iron metal: $$ \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) $$ (a) Balance this equation. (b) Calculate the number of grams of CO that can react with $$ 0.350 \mathrm{~kg} \text { of } \mathrm{Fe}_{2} \mathrm{O}_{3} $$ (c) Calculate the number of grams of Fe and the number of grams of \(\mathrm{CO}_{2}\) formed when \(0.350 \mathrm{~kg}\) of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) reacts. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

Calculate the following quantities: (a) mass, in grams, of 0.105 mole of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) (b) moles of \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\) in \(143.50 \mathrm{~g}\) of this substance (c) number of molecules in \(1.0 \times 10^{-6} \mathrm{~mol} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (d) number of \(\mathrm{N}\) atoms in \(0.410 \mathrm{~mol} \mathrm{NH}_{3}\)

(a) The characteristic odor of pineapple is due to ethyl butyrate, a compound containing carbon, hydrogen, and oxygen. Combustion of \(2.78 \mathrm{mg}\) of ethyl butyrate produces \(6.32 \mathrm{mg}\) of \(\mathrm{CO}_{2}\) and \(2.58 \mathrm{mg}\) of \(\mathrm{H}_{2} \mathrm{O}\). What is the empirical formula of the compound? (b) Nicotine, a component of tobacco, is composed of \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{N}\). A 5.250 -mg sample of nicotine was combusted, producing \(14.242 \mathrm{mg}\) of \(\mathrm{CO}_{2}\) and \(4.083 \mathrm{mg}\) of \(\mathrm{H}_{2} \mathrm{O}\). What is the empirical formula for nicotine? If nicotine has a molar mass of \(160 \pm 5 \mathrm{~g} / \mathrm{mol}\), what is its molecular formula?
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