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Chapter 22: Problem 17

Complete and balance the following equations: (a) \(\mathrm{NaOCH}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{CuO}(s)+\mathrm{HNO}_{3}(a q)\) (c) \(\mathrm{WO}_{3}(s)+\mathrm{H}_{2}(g) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{NH}_{2} \mathrm{OH}(l)+\mathrm{O}_{2}(g)\) (e) \(\mathrm{Al}_{4} \mathrm{C}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\)

Short Answer

Expert verified
The balanced chemical equations for the given reactions are: (a) \(\mathrm{NaOCH}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{NaOH}(aq) + \mathrm{CH}_{3}\mathrm{OH}(l)\) (b) \(\mathrm{CuO}(s) + 2\mathrm{HNO}_{3}(aq) \longrightarrow \mathrm{Cu(NO}_{3})_{2}(aq) + \mathrm{H}_{2}\mathrm{O}(l)\) (c) \(\mathrm{WO}_{3}(s) + 3\mathrm{H}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{W}(s) + 3 \mathrm{H}_{2}\mathrm{O}(g)\) (d) \(2\mathrm{NH}_{2} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{N}_{2}(g)\) (e) \(\mathrm{Al}_{4} \mathrm{C}_{3}(s) + 12\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 4\mathrm{Al(OH)}_{3}(s) + 3\mathrm{CH}_{4}(g)\)

Step by step solution

01

(a) Complete the equation

For equation (a), sodium methoxide (NaOCH3) reacts with water (H2O). The products of this reaction are sodium hydroxide (NaOH) and methanol (CH3OH). So, the completed equation is: \(\mathrm{NaOCH}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{NaOH}(aq) + \mathrm{CH}_{3}\mathrm{OH}(l)\) Now, we need to balance the equation.
02

(a) Balance the equation

In this case, the equation is already balanced: \[\mathrm{NaOCH}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{NaOH}(aq) + \mathrm{CH}_{3}\mathrm{OH}(l)\]
03

(b) Complete and balance the equation

For equation (b), copper oxide (CuO) reacts with nitric acid (HNO3). The products of this reaction are copper nitrate (Cu(NO3)2) and water (H2O). The completed equation is: \(\mathrm{CuO}(s) + \mathrm{HNO}_{3}(aq) \longrightarrow \mathrm{Cu(NO}_{3})_{2}(aq) + \mathrm{H}_{2}\mathrm{O}(l)\) Now, balance the equation by adding a 2 in front of HNO3: \[\mathrm{CuO}(s) + 2\mathrm{HNO}_{3}(aq) \longrightarrow \mathrm{Cu(NO}_{3})_{2}(aq) + \mathrm{H}_{2}\mathrm{O}(l)\]
04

(c) Complete and balance the equation

For equation (c), tungsten trioxide (WO3) reacts with hydrogen gas (H2) under heat, producing tungsten (W) and water (H2O). The completed equation is: \(\mathrm{WO}_{3}(s) + \mathrm{H}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{W}(s) + \mathrm{H}_{2}\mathrm{O}(g)\) Balance the equation by adding a 3 in front of H2O and a 3 in front of H2: \[\mathrm{WO}_{3}(s) + 3\mathrm{H}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{W}(s) + 3 \mathrm{H}_{2}\mathrm{O}(g)\]
05

(d) Complete and balance the equation

For equation (d), hydroxylamine (NH2OH) reacts with oxygen gas (O2) to produce water (H2O) and nitrogen gas (N2). The completed equation is: \(\mathrm{NH}_{2} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{N}_{2}(g)\) Balance the equation by adding coefficients as follows: \[2\mathrm{NH}_{2} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow 3\mathrm{H}_{2}\mathrm{O}(l) + \mathrm{N}_{2}(g)\]
06

(e) Complete and balance the equation

For equation (e), aluminum carbide (Al4C3) reacts with water (H2O) to produce aluminum hydroxide (Al(OH)3) and methane (CH4). The completed equation is: \(\mathrm{Al}_{4} \mathrm{C}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Al(OH)}_{3}(s) + \mathrm{CH}_{4}(g)\) Balance the equation by adding coefficients as follows: \[\mathrm{Al}_{4} \mathrm{C}_{3}(s) + 12\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 4\mathrm{Al(OH)}_{3}(s) + 3\mathrm{CH}_{4}(g)\]

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Most popular questions from this chapter

One method proposed for removing \(\mathrm{SO}_{2}\) from the flue gases of power plants involves reaction with aqueous \(\mathrm{H}_{2} \mathrm{~S}\). Elemental sulfur is the product. (a) Write a balanced chemical equation for the reaction. (b) What volume of \(\mathrm{H}_{2} \mathrm{~S}\) at \(27^{\circ} \mathrm{C}\) and 760 torr would be required to remove the \(\mathrm{SO}_{2}\) formed by burning 2.0 tons of coal containing \(3.5 \% \mathrm{~S}\) by mass? (c) What mass of elemental sulfur is produced? Assume that all reactions are \(100 \%\) efficient.

Explain the following observations: (a) The highest fluoride compound formed by nitrogen is \(\mathrm{NF}_{3}\), whereas phosphorus readily forms \(\mathrm{PF}_{5}\). (b) Although \(\mathrm{CO}\) is a well-known compound, SiO does not exist under ordinary conditions. (c) \(\mathrm{AsH}_{3}\) is a stronger reducing agent than \(\mathrm{NH}_{3} .\)

Write balanced equations for each of the following reactions. (a) When mercury(II) oxide is heated, it decomposes to form \(\mathrm{O}_{2}\) and mercury metal. (b) When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, \(\mathrm{PbS}(s)\), reacts with ozone to form \(\mathrm{PbSO}_{4}(s)\) and \(\mathrm{O}_{2}(g)\). (d) When heated in air, \(\mathrm{ZnS}(s)\) is converted to \(\mathrm{ZnO}\). (e) Potassium peroxide reacts (f) Oxygen with \(\mathrm{CO}_{2}(g)\) to give potassium carbonate and \(\mathrm{O}_{2}\). is converted to ozone in the upper atmosphere.

Complete and balance the following equations: (a) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow\) (c) \(\mathrm{MnO}_{2}(s)+\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{AlP}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (e) \(\mathrm{Na}_{2} \mathrm{~S}(s)+\mathrm{HCl}(a q) \longrightarrow\)

Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. (d) Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\). (e) Hydrazine reduces \(\mathrm{CrO}_{4}^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\) in base (hydrazine is oxidized to \(\mathrm{N}_{2}\) ).
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