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Chapter 22: Problem 66

Complete and balance the following equations: (a) \(\mathrm{CO}_{2}(g)+\mathrm{OH}^{-}(a q) \longrightarrow\) (b) \(\mathrm{NaHCO}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow\) (c) \(\mathrm{CaO}(s)+\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow}\) (d) $\mathrm{C}(s)+\mathrm{H}_{2} \mathrm{O}(g) \stackrel{\Delta}{\longrightarrow}$ (e) \(\mathrm{CuO}(s)+\mathrm{CO}(g) \longrightarrow\)

Short Answer

Expert verified
(a) \[\mathrm{CO}_{2}(g) + 2\,\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{3}^{2-}(a q)\] (b) \[\mathrm{NaHCO}_{3}(s) + \mathrm{H}^{+}(a q) \longrightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Na}^{+}(a q) + \mathrm{CO}_{2}(g)\] (c) \[\mathrm{CaO}(s) + 2\,\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{CaC}_{2}(s)\] (d) \[C(s) + \mathrm{H}_{2}\mathrm{O}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}(g) + \mathrm{H}_{2}(g)\] (e) \[\mathrm{CuO}(s) + \mathrm{CO}(g) \longrightarrow \mathrm{Cu}(s) + \mathrm{CO}_{2}(g)\]

Step by step solution

01

(a: Determine products and balance the equation)

For the first equation, we have carbon dioxide (CO₂) reacting with hydroxide ions (OH⁻). This reaction is an acid-base reaction, where CO₂ acts as an acidic oxide, and OH⁻ acts as a base. The products formed in this reaction will be water (H₂O) and a salt, which is a carbonate anion (CO₃²⁻) paired with an appropriate cation. Since OH⁻ contributes one H⁺ ion, the cation is H⁺. The balanced equation is: \[\mathrm{CO}_{2}(g) + 2\,\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{CO}_{3}^{2-}(a q)\]
02

(b: Determine products and balance the equation)

The second equation involves sodium bicarbonate (NaHCO₃) reacting with hydrogen ions (H⁺). This is another acid-base reaction, with NaHCO₃ acting as an amphoteric substance, meaning that it can act as an acid or a base. In this case, it's acting as a base. The products formed are water (H₂O) and sodium chloride (NaCl). The balanced equation is: \[\mathrm{NaHCO}_{3}(s) + \mathrm{H}^{+}(a q) \longrightarrow \mathrm{H}_{2}\mathrm{O}(l) + \mathrm{Na}^{+}(a q) + \mathrm{CO}_{2}(g)\]
03

(c: Determine products and balance the equation)

The third equation involves calcium oxide (CaO) reacting with carbon (C) at high temperature (∆). This is a redox reaction, which means that there is a transfer of electrons between reacting species. Calcium will reduce and absorb oxygen from calcium oxide, resulting in calcium carbide (CaC₂) as the product. To balance this equation, we need to ensure that there is the same number of atoms of each element on both sides. The balanced equation is: \[\mathrm{CaO}(s) + 2\,\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow} \mathrm{CaC}_{2}(s)\]
04

(d: Determine products and balance the equation)

The fourth equation involves carbon (C) reacting with water (H₂O) at high temperature (∆). This reaction is a gas-solid reaction, in which water participates as a reactant in the gas phase. The product of this reaction is gas synthesis, which is a mixture of hydrogen (H₂) and carbon monoxide (CO). To balance this equation, we need to adjust the stoichiometric coefficients. The balanced equation is: \[C(s) + \mathrm{H}_{2}\mathrm{O}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CO}(g) + \mathrm{H}_{2}(g)\]
05

(e: Determine products and balance the equation)

The last equation involves copper oxide (CuO) reacting with carbon monoxide (CO). This is another redox reaction, with copper oxide acting as an oxidizing agent and carbon monoxide acting as a reducing agent. The products of this reaction are copper (Cu) and carbon dioxide (CO₂). The balanced equation is: \[\mathrm{CuO}(s) + \mathrm{CO}(g) \longrightarrow \mathrm{Cu}(s) + \mathrm{CO}_{2}(g)\]

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Most popular questions from this chapter

Complete and balance the following equations: (a) \(\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{Al}_{2} \mathrm{O}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow\) (c) $\mathrm{Na}_{2} \mathrm{O}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (d) $\mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (e) \(\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (f) \(\mathrm{NO}(g)+\mathrm{O}_{3}(g) \longrightarrow\)

Give the chemical formula for (a) fullerene, (b) potassium cyanide, (c) zinc carbide, (d) zinc acetylide, (e) carbon disulfide.

Name the following compounds and assign oxidation states to the halogens in them: (a) \(\mathrm{BCl}_{3}\), (b) \(\mathrm{Sr}\left(\mathrm{IO}_{4}\right)_{2}\), (c) \(\mathrm{LiOCl}\) (d) \(\mathrm{HClO}\) (e) \(\mathrm{CuClO}\) (f) \(\mathrm{Mg}\left(\mathrm{IO}_{2}\right)\).

Indicate whether each of the following statements is true or false (a) \(\mathrm{H}_{2}(g)\) and \(\mathrm{D}_{2}(g)\) are allotropic forms of hydrogen. (b) \(\mathrm{ClF}_{3}\) is an interhalogen compound. (c) \(\mathrm{MgO}(s)\) is an acidic anhydride. (d) \(\mathrm{SO}_{2}(g)\) is an acidic anhydride. (e) $2 \mathrm{H}_{3} \mathrm{PO}_{4}(l) \rightarrow \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}(l)+\mathrm{H}_{2} \mathrm{O}(g)$ is an example of a condensation reaction. (f) Tritium is an isotope of the element hydrogen. (g) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g)\) is an example of a disproportionation reaction.

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q),(\mathbf{b})\) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+}\) (c) aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) to mercury metal. Write balanced equations for these reactions.
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