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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblem 105c3
Chapter 3, Problem 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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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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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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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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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Related Practice
Textbook Question

(b) Because atoms are spherical, they cannot occupy all of the space of the cube. The silver atoms pack in the solid in such a way that 74% of the volume of the solid is actually filled with the silver atoms. Calculate the volume of a single silver atom.

Textbook Question

A mixture of N21g2 and H21g2 reacts in a closed container to form ammonia, NH31g2. The reaction ceases before either reactant has been totally consumed. At this stage 3.0 mol N2, 3.0 mol H2, and 3.0 mol NH3 are present. How many moles of N2 and H2 were present originally?

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Textbook Question

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 C2H2 are present after the reaction is complete?

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Textbook Question

The fat stored in a camel's hump is a source of both energy and water. Calculate the mass of H2O produced by the metabolism of 1.0 kg of fat, assuming the fat consists entirely of tristearin 1C57H110O62, a typical animal fat, and assuming that during metabolism, tristearin reacts with O2 to form only CO2 and H2O.

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