Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 87

Write balanced chemical equations for \((\mathbf{a})\) the complete combustion of acetone \(\left(\mathrm{CH}_{3} \mathrm{COCH}_{3}\right),\) a common organic solvent; (b) the decomposition of solid mercury (I) carbonate into carbon dioxide gas, mercury, and solid mercury oxide; (c) the combination reaction between sulphur dioxide gas and liquid water to produce sulfurous acid.

Short Answer

Expert verified
a) Balanced equation for the complete combustion of acetone: \(CH_3COCH_3 + 4O_2 → 3CO_2 + 3H_2O\) b) Balanced equation for the decomposition of solid mercury(I) carbonate: \(Hg_2CO_3 → CO_2 + 2Hg + 2HgO\) c) Balanced equation for the combination reaction between sulfur dioxide gas and liquid water: \(SO_2 + H_2O → H_2SO_3\)

Step by step solution

01

a) Combustion of acetone

Write the initial reaction equation: Acetone (CH₃COCH₃) reacts with oxygen gas (O₂) to produce carbon dioxide (CO₂) and water (H₂O). Unbalanced equation: CH₃COCH₃ + O₂ → CO₂ + H₂O Balancing the equation by adjusting the coefficients: 1. We have 6 hydrogen atoms on the left side of the equation, so we should have 3 H₂O molecules on the right side. 2. We have 3 carbon atoms on the left side of the equation, so we should have 3 CO₂ molecules on the right side. 3. Now, we need to balance the oxygen atoms. We have 4 oxygen atoms from the 2 O₂ molecules on the left and a total of 9 oxygen atoms on the right. Balanced equation: CH₃COCH₃ + 4O₂ → 3CO₂ + 3H₂O
02

b) Decomposition of mercury(I) carbonate

Write the initial reaction equation: Solid mercury(I) carbonate (Hg₂CO₃) decomposes into carbon dioxide gas (CO₂), mercury (Hg), and solid mercury oxide (HgO). Unbalanced equation: Hg₂CO₃ → CO₂ + Hg + HgO Balancing the equation by adjusting the coefficients: 1. We need 2 mercury atoms on the right side of the equation, so we place a 2 in front of Hg. 2. This results in 3 mercury atoms on the right side, so we place a 2 in front of HgO to balance the equation. Balanced equation: Hg₂CO₃ → CO₂ + 2Hg + 2HgO
03

c) Combination of sulfur dioxide and water

Write the initial reaction equation: Sulfur dioxide gas (SO₂) reacts with liquid water (H₂O) to produce sulfurous acid (H₂SO₃). Unbalanced equation: SO₂ + H₂O → H₂SO₃ There's no need to balance this particular reaction, as the coefficients in the unbalanced equation are already correct for balancing the atoms on both sides of the reaction. Balanced equation: SO₂ + H₂O → H₂SO₃

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The allowable concentration level of vinyl chloride, $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl},\( in the atmosphere in a chemical plant is \)2.0 \times 10^{-6} \mathrm{~g} / \mathrm{L}$. How many moles of vinyl chloride in each liter does this represent? How many molecules per liter?

(a) Define the terms limiting reactant and excess reactant. (b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant? (c) Why should you base your choice of which compound is the limiting reactant on its number of initial moles, not on its initial mass in grams?

Write a balanced chemical equation for the reaction that occurs when (a) \(\mathrm{Mg}(s)\) reacts with \(\mathrm{Cl}_{2}(g) ;(\mathbf{b})\) barium carbonate decomposes into barium oxide and carbon dioxide gas when heated; \((\mathbf{c})\) the hydrocarbon styrene, \(\mathrm{C}_{8} \mathrm{H}_{8}(l),\) is combusted in air; \((\mathbf{d})\) dimethylether, $\mathrm{CH}_{3} \mathrm{OCH}_{3}(g),$ is combusted in air.

Aluminum hydroxide reacts with sulfuric acid as follows: $2 \mathrm{Al}(\mathrm{OH})_{3}(s)+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l)\( Which is the limiting reactant when \)0.500 \mathrm{~mol} \mathrm{Al}(\mathrm{OH})_{3}\( and \)0.500 \mathrm{~mol} \mathrm{H}_{2} \mathrm{SO}_{4}$ are allowed to react? How many moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) can form under these conditions? How many moles of the excess reactant remain after the completion of the reaction?

Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write the balanced chemical equation for this reaction. (b) How many grams of aluminum hydroxide are obtained from \(14.2 \mathrm{~g}\) of aluminum sulfide?
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free