Write the balanced chemical equations for (a) the complete combustion of acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right),\) the main ingredient in vinegar; (b) the decomposition of solid calcium hydroxide into solid calcium oxide (lime) and water vapor; (c) the combination reaction between nickel metal and chlorine gas.

Short Answer

Expert verified
The balanced chemical equations for the given reactions are: (a) Complete combustion of acetic acid: \( 2 \, \text{CH}_{3}\text{COOH} \) + \( O_{2} \) → \( 2 \, \text{CO}_{2} \) + \( 2 \, H_{2}O \) (b) Decomposition of solid calcium hydroxide: Ca(OH)₂ → CaO + H₂O (c) Combination reaction between nickel metal and chlorine gas: Ni+ Cl₂ → NiCl₂

Step by step solution

01

Reaction (a) Complete combustion of acetic acid (CH₃COOH)

The reactants for this reaction are acetic acid (CH₃COOH) and oxygen (O₂). The complete combustion of an organic compound like acetic acid produces carbon dioxide (CO₂) and water (H₂O). Let's write the unbalanced equation showing the reactants and products: CH₃COOH + O₂ → CO₂ + H₂O Now, let's balance the equation by adjusting the coefficients in front of each molecule: \( 2 \, \text{CH}_{3}\text{COOH} \) + \( O_{2} \) → \( 2 \, \text{CO}_{2} \) + \( 2 \, H_{2}O \) Checking the balance of atoms: C: 2 on the left and 2 on the right H: 4 on the left and 4 on the right O: 4 on the left and 4 on the right The balanced chemical equation for the complete combustion of acetic acid is: \( 2 \, \text{CH}_{3}\text{COOH} \) + \( O_{2} \) → \( 2 \, \text{CO}_{2} \) + \( 2 \, H_{2}O \)
02

Reaction (b) Decomposition of solid calcium hydroxide

The reactant for this reaction is solid calcium hydroxide (Ca(OH)₂). The decomposition reaction will produce solid calcium oxide (CaO) and water vapor (H₂O). Let's write the unbalanced equation: Ca(OH)₂ → CaO + H₂O The equation is already balanced as there's the same number of atoms for each element on both sides. The balanced chemical equation for the decomposition of solid calcium hydroxide is: Ca(OH)₂ → CaO + H₂O
03

Reaction (c) Combination reaction between nickel metal and chlorine gas

The reactants for this reaction are nickel metal (Ni) and chlorine gas (Cl₂). The combination reaction produces nickel chloride (NiCl₂). Let's write the unbalanced equation: Ni + Cl₂ → NiCl₂ The equation is already balanced as the same number of atoms for each element is present on both sides. The balanced chemical equation for the combination reaction between nickel metal and chlorine gas is: Ni + Cl₂ → NiCl₂

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.

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

Hydrogen sulfide is an impurity in natural gas that must be removed. One common removal method is called the Claus process, which relies on the reaction: $$ 8 \mathrm{H}_{2} \mathrm{S}(g)+4 \mathrm{O}_{2}(g) \longrightarrow \mathrm{S}_{8}(l)+8 \mathrm{H}_{2} \mathrm{O}(g) $$ Under optimal conditions the Claus process gives 98\(\%\) yield of \(S_{8}\) from \(\mathrm{H}_{2}\) . If you started with 30.0 g of \(\mathrm{H}_{2} \mathrm{S}\) and 50.0 \(\mathrm{g}\) of \(\mathrm{O}_{2},\) how many grams of \(\mathrm{S}_{8}\) would be produced, assuming 98\(\%\) yield?

Hydrogen cyanide, HCN, is a poisonous gas. The lethal dose is approximately 300 \(\mathrm{mg}\) HCN per kilogram of air when inhaled. (a) Calculate the amount of HCN that gives the lethal dose in a small laboratory room measuring \(12 \times 15 \times 8.0 \mathrm{ft}\) . The density of air at \(26^{\circ} \mathrm{C}\) is 0.00118 \(\mathrm{g} / \mathrm{cm}^{3} .\) (b) If the HCN is formed by reaction of \(\mathrm{NaCN}\) with an acid such as \(\mathrm{H}_{2} \mathrm{SO}_{4}\) what mass of NaCN gives the lethal dose in the room? $$ 2 \mathrm{NaCN}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{HCN}(g) $$ (c) HCN forms when synthetic fibers containing Orlon or Acrilan burn. Acrilan has an empirical formula of \(\mathrm{CH}_{2} \mathrm{CHCN},\) so HCN is 50.9\(\%\) of the formula by mass. A rug measures \(12 \times 15 \mathrm{ft}\) and contains 30 oz of Acrilan fibers per square yard of carpet. If the rug burns, will a lethal dose of HCN be generated in the room? Assume that the yield of HCN from the fibers is 20\(\%\) and that the carpet is 50\(\%\) consumed.

The semiconductor gallium arsenide, GaAs, is used in high-speed integrated circuits, light-emitting diodes, and solar cells. Its density is 5.32 \(\mathrm{g} / \mathrm{m}^{3} .\) It can be made by reacting trimethylgallium, \(\left(\mathrm{CH}_{3}\right)_{3} \mathrm{Ga},\) with arsine gas, \(\mathrm{AsH}_{3}\) . The other product of the reaction is methane, \(\mathrm{CH}_{4}\) . (a) If you reacted 450.0 g of trimethylgallium with 300.0 \(\mathrm{g}\) of arsine, what mass of GaAs could you make? (b) Which reactant, if any, would be left over, and how many moles of the leftover reactant would remain? (c) One application of GaAs uses it as a thin film. If you take the mass of GaAs from part (a) and make a 40 -nm thin film from it, what area, in \(\mathrm{cm}^{2},\) would it cover? Recall that \(1 \mathrm{nm}=1 \times 10^{-9} \mathrm{m} .\)

What is the molecular formula of each of the following compounds? $$ \begin{array}{l}{\text { (a) empirical formula } \mathrm{CH}_{2}, \text { molar mass }=84.0 \mathrm{g} / \mathrm{mol}} \\ {\text { (b) empirical formula } \mathrm{NH}_{2} \mathrm{Cl} \text { , molar mass }=51.5 \mathrm{g} / \mathrm{mol}}\end{array} $$

The combustion of one mole of liquid ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) , produces 1367 \(\mathrm{kJ}\) of heat. Calculate how much heat is produced when 235.0 \(\mathrm{g}\) of ethanol are combusted.

See all solutions

Recommended explanations on Chemistry Textbooks

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