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Chapter 3: Problem 16

(a) Determine the chemical formula of the product formed when the metallic element aluminum combines with the nonmetallic element bromine, \(\mathrm{Br}_{2}\). Write the balanced chemical equation for the reaction. (b) What products form when a compound containing \(\mathrm{C}, \mathrm{H},\) and \(\mathrm{O}\) is completely combusted in air? Write a balanced chemical equation for the combustion of acetone, \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l),\) in air.

Short Answer

Expert verified
The product formed when aluminum combines with bromine is AlBr₃, and the balanced chemical equation for the reaction is \(2 \mathrm{Al}(s) + 3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{AlBr}_{3}(s)\). When a compound containing C, H, and O is completely combusted in air, the products are carbon dioxide (CO₂) and water (H₂O). The balanced chemical equation for the combustion of acetone (\(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l)\)) is \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l) + 4 \mathrm{O}_{2}(g) \rightarrow 3 \mathrm{CO}_{2}(g) + 3 \mathrm{H}_{2}\mathrm{O}(l)\).

Step by step solution

01

Determine the ions formed by each element

Aluminum is a metal and forms a positive ion with a charge of +3 (Al³⁺) in a chemical reaction. Bromine is a non-metal and forms a negative ion with a charge of -1 (Br⁻) in a chemical reaction. Step 2: Combine the ions to form a compound
02

Write the chemical formula of the product

Since Al³⁺ has a charge of +3 and Br⁻ has a charge of -1, we need three Br⁻ ions to balance the charge of one Al³⁺ ion. Hence, the chemical formula of the compound formed is AlBr₃. Step 3: Write the balanced chemical equation
03

Write the balanced chemical equation for Al reacting with Br₂

The balanced chemical equation is: \[2 \mathrm{Al}(s) + 3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{AlBr}_{3}(s)\] For the second part of the exercise: Step 1: Determine the products of combustion
04

Identify the products of combustion

When compounds containing carbon, hydrogen, and oxygen are combusted in air, the products formed are carbon dioxide (CO₂) and water (H₂O). Step 2: Write the balanced chemical equation for the combustion of acetone
05

Write the balanced chemical equation for \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l)\)

The balanced chemical equation for the combustion of acetone is: \[\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l) + 4 \mathrm{O}_{2}(g) \rightarrow 3 \mathrm{CO}_{2}(g) + 3 \mathrm{H}_{2}\mathrm{O}(l)\]

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Most popular questions from this chapter

A particular coal contains \(2.5 \%\) sulfur by mass. When this coal is burned at a power plant, the sulfur is converted into sulfur dioxide gas, which is a pollutant. To reduce sulfur dioxide emissions, calcium oxide (lime) is used. The sulfur dioxide reacts with calcium oxide to form solid calcium sulfite. (a) Write the balanced chemical equation for the reaction. (b) If the coal is burned in a power plant that uses 2000 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide? (c) How many grams of calcium sulfite are produced daily by this power plant?

An organic compound was found to contain only \(\mathrm{C}, \mathrm{H},\) and Cl. When a 1.50 -g sample of the compound was completely combusted in air, \(3.52 \mathrm{~g}\) of \(\mathrm{CO}_{2}\) was formed. In a separate experiment the chlorine in a 1.00 -g sample of the compound was converted to \(1.27 \mathrm{~g}\) of AgCl. Determine the empirical formula of the compound.

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) \(\mathrm{PbCO}_{3}(s) \longrightarrow \mathrm{PbO}(s)+\mathrm{CO}_{2}(g)\) (b) \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (c) \(\mathrm{Mg}(s)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Mg}_{3} \mathrm{~N}_{2}(s)\) (d) \(\mathrm{C}_{7} \mathrm{H}_{8} \mathrm{O}_{2}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) (e) \(\mathrm{Al}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{AlCl}_{3}(s)\)

(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?

The source of oxygen that drives the internal combustion engine in an automobile is air. Air is a mixture of gases, principally \(\mathrm{N}_{2}(\sim 79 \%)\) and \(\mathrm{O}_{2}(\sim 20 \%) .\) In the cylinder of an automobile engine, nitrogen can react with oxygen to produce nitric oxide gas, NO. As \(\mathrm{NO}\) is emitted from the tailpipe of the car, it can react with more oxygen to produce nitrogen dioxide gas. (a) Write balanced chemical equations for both reactions. (b) Both nitric oxide and nitrogen dioxide are pollutants that can lead to acid rain and global warming; collectively, they are called " \(\mathrm{NO}_{\mathrm{x}}^{\prime \prime}\) gases. In \(2007,\) the United States emitted an estimated 22 million tons of nitrogen dioxide into the atmosphere. How many grams of nitrogen dioxide is this? (c) The production of \(\mathrm{NO}_{\mathrm{x}}\) gases is an unwanted side reaction of the main engine combustion process that turns octane, \(\mathrm{C}_{8} \mathrm{H}_{18}\), into \(\mathrm{CO}_{2}\) and water. If \(85 \%\) of the oxygen in an engine is used to combust octane and the remainder used to produce nitrogen dioxide, calculate how many grams of nitrogen dioxide would be produced during the combustion of 500 grams of octane.
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