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Chapter 22: Problem 69

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.

Short Answer

Expert verified
(a) \( 2CH_4 + 2 NH_3 + 3 O_2 \rightarrow 2 HCN + 6 H_2O \) (b) \( NaHCO_3 + HCl \rightarrow NaCl + CO_2 + H_2O \) (c) \( BaCO_3 + SO_2 \rightarrow BaSO_4 + CO_2 \)

Step by step solution

01

Write the unbalanced equation

First, we will write the unbalanced chemical equation for the reaction using the given information: \( CH_4 + NH_3 + O_2 \rightarrow HCN + H_2O \)
02

Balance the equation

Now, we will balance the chemical equation by adjusting the coefficients of the reactants and products. Balance the elements in the following order: C, H, N, and O. \[ 2CH_4 + 2 NH_3 + 3 O_2 \rightarrow 2 HCN + 6 H_2O \] The balanced equation for the formation of hydrogen cyanide is: \( 2CH_4 + 2 NH_3 + 3 O_2 \rightarrow 2 HCN + 6 H_2O \) (b) Reaction between baking soda and an acid:
03

Write the unbalanced equation

First, we will write the unbalanced chemical equation for the reaction using the given information. Baking soda is sodium bicarbonate (NaHCO3) and a common acid is hydrochloric acid (HCl). The products are sodium chloride (NaCl), carbon dioxide (CO2), and water (H2O). \( NaHCO_3 + HCl \rightarrow NaCl + CO_2 + H_2O \)
04

Balance the equation

This equation is already balanced as written. All elements have the same number of atoms on both sides of the equation. The balanced equation for the reaction between baking soda and an acid is: \( NaHCO_3 + HCl \rightarrow NaCl + CO_2 + H_2O \) (c) Reaction of barium carbonate with sulfur dioxide:
05

Write the unbalanced equation

First, we will write the unbalanced chemical equation for the reaction using the given information. Barium carbonate is BaCO3 and sulfur dioxide is SO2. The products are barium sulfate (BaSO4) and carbon dioxide (CO2). \( BaCO_3 + SO_2 \rightarrow BaSO_4 + CO_2 \)
06

Balance the equation

This equation is already balanced as written. All elements have the same number of atoms on both sides of the equation. The balanced equation for the reaction of barium carbonate with sulfur dioxide is: \( BaCO_3 + SO_2 \rightarrow BaSO_4 + CO_2 \)

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Most popular questions from this chapter

(a) What is the oxidation state of \(\mathrm{P}\) in \(\mathrm{PO}_{4}{ }^{3-}\) and of \(\mathrm{N}^{-}\)in \(\mathrm{NO}_{3}{ }^{-}\)? (b) Why doesn't N form a stable \(\mathrm{NO}_{4}^{3-}\). ion analogous to \(\mathrm{P}\) ?

Although the \(\mathrm{ClO}_{4}^{-}\)and \(\mathrm{IO}_{4}^{-}\)ions have been known for a long time, \(\mathrm{BrO}_{4}^{-}\)was not synthesized until 1965 . The ion was synthesized by oxidizing the bromate ion with xenon difluoride, producing xenon, hydrofluoric acid, and the perbromate ion. (a) Write the balanced equation for this reaction. (b) What are the oxidation states of Br in the Br-containing species in this reaction?

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.)

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 \(\mathrm{Cl}^{-}\). Nitrogen and the Other Group 5A Elements (Sections 22.7 and 22.8)

Write complete balanced half-reactions for (a) oxidation of nitrous acid to nitrate ion in acidic solution, (b) oxidation of \(\mathrm{N}_{2}\) to \(\mathrm{N}_{2} \mathrm{O}\) in acidic solution.
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