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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 105c3
Capitolo 3, Problema 105c3

When a mixture of 10.0 g of acetylene (C2H2) and 10.0 g of oxygen (O2) is ignited, the resulting combustion reaction produces CO2 and H2O. (c) How many grams of CO2 and H2O are present after the reaction is complete?

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1
Determine the molar mass of acetylene (C2H2) and oxygen (O2).
Calculate the moles of acetylene and oxygen initially present using their respective molar masses.
Write the balanced chemical equation for the combustion of acetylene: 2 C2H2 + 5 O2 ightarrow 4 CO2 + 2 H2O.
Using stoichiometry, determine the limiting reactant by comparing the mole ratio from the balanced equation with the moles of each reactant calculated.
Calculate the moles of CO2 produced based on the moles of the limiting reactant, then convert these moles of CO2 to grams using the molar mass of CO2.

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Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. In this case, understanding the stoichiometric ratios of acetylene and oxygen will help determine how much carbon dioxide is produced.
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Stoichiometry Concept

Combustion Reactions

Combustion reactions are exothermic reactions that occur when a substance reacts with oxygen, producing heat and light. In the case of acetylene (C2H2), it combusts in the presence of oxygen to form carbon dioxide (CO2) and water (H2O). Recognizing the products of the combustion of acetylene is essential for calculating the mass of CO2 produced.
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Combustion Apparatus

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between grams of a substance and moles, which are used in stoichiometric calculations. For this problem, knowing the molar masses of acetylene, oxygen, carbon dioxide, and water will facilitate the conversion of the initial masses into moles, allowing for the determination of the final mass of CO2 produced.
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Molar Mass Concept
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A mixture containing KClO3, K2CO3, KHCO3, and KCl was heated, producing CO2, O2, and H2O gases according to the following equations: 2 KClO31s2¡2 KCl1s2 + 3 O21g2 2 KHCO31s2¡K2O1s2 + H2O1g2 + 2 CO21g2 K2CO31s2¡K2O1s2 + CO21g2 The KCl does not react under the conditions of the reaction. If 100.0 g of the mixture produces 1.80 g of H2O, 13.20 g of CO2, and 4.00 g of O2, what was the composition of the original mixture? (Assume complete decomposition of the mixture.) How many grams of K2CO3 were in the original mixture?

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