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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) \(\mathrm{CuO}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\) (c) \(\mathrm{WO}_{3}(s)+\mathrm{H}_{2}(g) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{NH}_{2} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow\) (e) $\mathrm{Al}_{4} \mathrm{C}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$

Short Answer

Expert verified
(a) NaOCH3(s) + H2O(l) → NaOH(aq) + CH3OH(l) (b) CuO(s) + 2 HNO3(aq) → Cu(NO3)2(aq) + H2O(l) (c) WO3(s) + 3 H2(g) → W(s) + 3 H2O(l) (d) 4 NH2OH(l) + 3 O2(g) → 2 N2(g) + 6 H2O(l) (e) Al4C3(s) + 12 H2O(l) → 4 Al(OH)3(s) + 3 CH4(g)

Step by step solution

01

(a) Balancing NaOCH3(s) + H2O(l) → ?

First, we need to complete the equation by identifying the products formed. In this reaction, sodium methoxide (NaOCH3) acts as a base, and water (H2O) acts as an acid. Sodium hydroxide (NaOH) and methanol (CH3OH) are formed as products. Now, we can balance the equation: NaOCH3(s) + H2O(l) → NaOH(aq) + CH3OH(l) The equation is already balanced with equal numbers of atoms for each element on both sides.
02

(b) Balancing CuO(s) + HNO3(aq) → ?

Copper(II) oxide (CuO) reacts with nitric acid (HNO3) in an acid-base reaction, forming copper(II) nitrate (Cu(NO3)2) and water (H2O) as products. Now, we can balance the equation: CuO(s) + 2 HNO3(aq) → Cu(NO3)2(aq) + H2O(l)
03

(c) Balancing WO3(s) + H2(g) → ?

Tungsten(VI) oxide (WO3) reacts with hydrogen gas (H2) in a reduction reaction. The products are tungsten metal (W) and water (H2O). Now, we can balance the equation by using a heat symbol (∆) to denote that heat is applied to the reaction: WO3(s) + 3 H2(g) → W(s) + 3 H2O(l)
04

(d) Balancing NH2OH(l) + O2(g) → ?

Hydroxylamine (NH2OH) reacts with oxygen gas (O2) in a combustion reaction. The products are nitrogen gas (N2) and water (H2O). Balanced combustion reactions typically have whole-number coefficients. Now, we can balance the equation: 2 NH2OH(l) + 3/2 O2(g) → N2(g) + 3 H2O(l) To make all coefficients whole numbers, we can multiply the whole equation by 2: 4 NH2OH(l) + 3 O2(g) → 2 N2(g) + 6 H2O(l)
05

(e) Balancing Al4C3(s) + H2O(l) → ?

Aluminum carbide (Al4C3) reacts with water (H2O) to form aluminum hydroxide (Al(OH)3) and methane gas (CH4) as products. Now, we can balance the equation: Al4C3(s) + 12 H2O(l) → 4 Al(OH)3(s) + 3 CH4(g)

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Most popular questions from this chapter

Write a balanced equation for each of the following reactions: (a) preparation of white phosphorus from calcium phosphate, (b) hydrolysis of \(\mathrm{PBr}_{3}\), (c) reduction of \(\mathrm{PBr}_{3}\) to \(\mathrm{P}_{4}\) in the gas phase, using \(\mathrm{H}_{2}\).

Write a balanced equation for each of the following reactions: (a) Hydrogen cyanide is formed commercially by passing a mixture of methane, ammonia, and air over a catalyst at \(800^{\circ} \mathrm{C}\). Water is a by-product of the reaction. (b) Baking soda reacts with acids to produce carbon dioxide gas. (c) When barium carbonate reacts in air with sulfur dioxide, barium sulfate and carbon dioxide form.

Borazine, \((\mathrm{BH})_{3}(\mathrm{NH})_{3},\) is an analog of \(\mathrm{C}_{6} \mathrm{H}_{6},\) benzene. It can be prepared from the reaction of diborane with ammonia, with hydrogen as another product; or from lithium borohydride and ammonium chloride, with lithium chloride and hydrogen as the other products. (a) Write balanced chemical equations for the production of borazine using both synthetic methods. (b) Draw the Lewis dot structure of borazine. (c) How many grams of borazine can be prepared from $2.00 \mathrm{~L}$ of ammonia at STP, assuming diborane is in excess?

Write a balanced equation for each of the following reactions: (a) hydrolysis of \(\mathrm{PCl}_{5},(\mathbf{b})\) dehydration of phosphoric acid (also called orthophosphoric acid) to form pyrophosphoric acid, \((\mathbf{c})\) reaction of \(\mathrm{P}_{4} \mathrm{O}_{10}\) with water.

(a) The \(\mathrm{P}_{4}, \mathrm{P}_{4} \mathrm{O}_{6}\) and $\mathrm{P}_{4} \mathrm{O}_{10}$ molecules have a common structural feature of four \(\mathrm{P}\) atoms arranged in a tetrahedron (Figures 22.27 and 22.28 ). Does this mean that the bonding between the \(\mathrm{P}\) atoms is the same in all these cases? Explain. (b) Sodium trimetaphosphate $\left(\mathrm{Na}_{3} \mathrm{P}_{3} \mathrm{O}_{9}\right)$ and sodium tetrametaphosphate \(\left(\mathrm{Na}_{4} \mathrm{P}_{4} \mathrm{O}_{12}\right)\) are used as water-softening agents. They contain cyclic $\mathrm{P}_{3} \mathrm{O}_{9}^{3-}\( and \)\mathrm{P}_{4} \mathrm{O}_{12}{ }^{4-}$ ions, respectively. Propose reasonable structures for these ions.
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