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Chapter 22: Problem 68

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
The short answer is: (a) CO₂(g) + OH⁻(aq) → HCO₃⁻(aq) (b) NaHCO₃(s) + H⁺(aq) → Na⁺(aq) + CO₂(g) + H₂O(l) (c) CaO(s) + 2 C(s) → CaC₂(s) (d) C(s) + H₂O(g) → CO(g) + H₂(g) (e) CuO(s) + CO(g) → Cu(s) + CO₂(g)

Step by step solution

01

(Identify Products)

For the first reaction, CO₂(g) + OH⁻(aq) react together. The possible product of this reaction is the formation of bicarbonate ion, HCO₃⁻(aq) since hydrogen from OH⁻ would bond to CO₂. \ #a) Balancing the Reaction#
02

(Balance Atoms)

To balance the equation, adjust the coefficients: \( \) 1 CO₂(g) + 1 OH⁻(aq) → 1 HCO₃⁻(aq) \ Here, the number of atoms for each element is the same on both sides of the equation. Thus, the balanced equation is: \( \) CO₂(g) + OH⁻(aq) → HCO₃⁻(aq) #b) Completing the Reaction#
03

(Identify Products)

For the second reaction, NaHCO₃(s) + H⁺(aq) react together. The possible products of this reaction are Na⁺(aq), CO₂(g), and H₂O(l) because the H⁺ would bond with the HCO₃⁻ to form water and release carbon dioxide. \ #b) Balancing the Reaction#
04

(Balance Atoms)

To balance the equation, adjust the coefficients: \( \) 1 NaHCO₃(s) + 1 H⁺(aq) → 1 Na⁺(aq) + 1 CO₂(g) + 1 H₂O(l) \ Here, the number of atoms for each element is the same on both sides of the equation. Thus, the balanced equation is: \( \) NaHCO₃(s) + H⁺(aq) → Na⁺(aq) + CO₂(g) + H₂O(l) #c) Completing the Reaction#
05

(Identify Products)

For the third reaction, CaO(s) + C(s) react together with Δ (heat). The possible product of this reaction is the formation of calcium carbide, CaC₂(s), because calcium would bond with carbon. \( \) #c) Balancing the Reaction#
06

(Balance Atoms)

To balance the equation, adjust the coefficients: \( \) 1 CaO(s) + 2 C(s) → 1 CaC₂(s) \ Here, the number of atoms for each element is the same on both sides of the equation. Thus, the balanced equation is: \( \) CaO(s) + 2 C(s) → CaC₂(s) #d) Completing the Reaction#
07

(Identify Products)

For the fourth reaction, C(s) + H₂O(g) react together with Δ (heat). The possible product of this reaction is the formation of carbon monoxide, CO(g) and hydrogen gas, H₂(g) since carbon would bond with oxygen and hydrogen is released as a gas. \( \) #d) Balancing the Reaction#
08

(Balance Atoms)

To balance the equation, adjust the coefficients: \( \) 1 C(s) + 1 H₂O(g) → 1 CO(g) + 1 H₂(g) \ Here, the number of atoms for each element is the same on both sides of the equation. Thus, the balanced equation is: \( \) C(s) + H₂O(g) → CO(g) + H₂(g) #e) Completing the Reaction#
09

(Identify Products)

For the fifth reaction, CuO(s) + CO(g) react together. The possible product of this reaction is the formation of copper, Cu(s) and carbon dioxide, CO₂(g) as carbon would bond with the oxygen bound to copper. \ #e) Balancing the Reaction#
10

(Balance Atoms)

To balance the equation, adjust the coefficients: \( \) 1 CuO(s) + 1 CO(g) → 1 Cu(s) + 1 CO₂(g) \ Here, the number of atoms for each element is the same on both sides of the equation. Thus, the balanced equation is: \( \) CuO(s) + CO(g) → Cu(s) + CO₂(g)

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Most popular questions from this chapter

Write a balanced equation for each of the following reactions. (You may have to guess at one or more of the reaction products, but you should be able to make a reasonable guess, based on your study of this chapter.) (a) Hydrogen selenide can be prepared by reaction of an aqueous acid solution on aluminum selenide. (b) Sodium thiosulfate is used to remove excess \(\mathrm{Cl}_{2}\) from chlorine-bleached fabrics. The thiosulfate ion forms \(\mathrm{SO}_{4}^{2-}\) and elemental sulfur, while \(\mathrm{Cl}_{2}\) is reduced to \(\mathrm{Cl}^{-}\).

Predict whether each of the following oxides is acidic, basic, , (d) \(\mathrm{CaO}\) amphoteric, or neutral: (a) \(\mathrm{NO}_{2},\) (b) \(\mathrm{CO}_{2},\) (c) \(\mathrm{Al}_{2} \mathrm{O}_{3}\),

Name the following compounds and assign oxidation states to (a) \(\mathrm{Fe}\left(\mathrm{ClO}_{3}\right)_{3}\) (c) \(\mathrm{XeF}_{6}\) the halogens in them: (b) \(\mathrm{HClO}_{2}\) (d) \(\mathrm{BrF}_{5}\) (e) \(\mathrm{XeOF}_{4}\), (f) \(\mathrm{HIO}_{3}\)

Both dimethylhydrazine, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{NNH}_{2}\), and methylhydrazine, \(\mathrm{CH}_{3} \mathrm{NHNH}_{2}\), have been used as rocket fuels. When dinitrogen tetroxide \(\left(\mathrm{N}_{2} \mathrm{O}_{4}\right)\) is used as the oxidizer, the products are \(\mathrm{H}_{2} \mathrm{O}\) \(\mathrm{CO}_{2}\), and \(\mathrm{N}_{2}\). If the thrust of the rocket depends on the volume of the products produced, which of the substituted hydrazines produces a greater thrust per gram total mass of oxidizer plus fuel? [Assume that both fuels generate the same temperature and that \(\mathrm{H}_{2} \mathrm{O}(g)\) is formed. \(]\)

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) \(\mathrm{Na}_{2} \mathrm{~S}(s)+\mathrm{HCl}(a q) \longrightarrow\)
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