Chapter 13: Problem 34
The following reaction occurs when a burner on a gas stove is lit: \(\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\)
Short Answer
Expert verified
The balanced chemical equation for the combustion of methane (CH4) with oxygen (O2) forms carbon dioxide (CO2) and water (H2O) and is already correctly balanced.
Step by step solution
01
Write the Balance Equation
Verify that the chemical equation is balanced by counting atoms of each element on the reactant and product sides of the equation. For the given reaction, the number of atoms for each element are: Carbon (C): 1 on both sides; Hydrogen (H): 4 on both sides; Oxygen (O): 4 on both sides (2 from the two O2 molecules and 2 from the CO2 and 2 H2O molecules). The reaction is already balanced.
02
Identify the Reaction Type
Determine the type of reaction taking place. In this case, methane (CH4) is reacting with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). This is a combustion reaction, which is a type of exothermic reaction where a hydrocarbon fuel reacts with oxygen to produce carbon dioxide, water, and heat.
03
Describe the Reaction Process
When a burner on a gas stove is lit, the methane gas (CH4) comes in contact with oxygen (O2) in the air. This mixture is ignited, causing the methane to combust, which converts the reactants into carbon dioxide (CO2) and water (H2O) in the form of steam while releasing heat.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Balancing Chemical Equations
Understanding how to balance chemical equations is a fundamental skill in chemistry. Balanced equations are essential because they show that mass is conserved during a reaction as per the Law of Conservation of Mass. For a chemical equation to be balanced, the number of atoms for each element must be the same on both the reactant and product sides. In the combustion of methane, the balanced equation is \(\mathrm{CH}_{4}(g) + 2 \mathrm{O}_{2}(g) \rightleftharpoons \mathrm{CO}_{2}(g) + 2 \mathrm{H}_{2} \mathrm{O}(g)\).Counting the atoms, we see: For carbon (C), there's 1 atom on each side; for hydrogen (H), there are 4 on each side; and for oxygen (O), we have a total of 4 atoms on each side, demonstrating that the equation is balanced. Knowing how to balance equations helps with understanding other concepts such as stoichiometry in chemical reactions.
When balancing equations, start by listing the elements and their count on both sides. Balance the elements one at a time, adjusting coefficients—a numerical front of chemical formulas—while avoiding altering subscripts in formulas, as that changes the chemicals themselves.
When balancing equations, start by listing the elements and their count on both sides. Balance the elements one at a time, adjusting coefficients—a numerical front of chemical formulas—while avoiding altering subscripts in formulas, as that changes the chemicals themselves.
Characteristics of Exothermic Reactions
Exothermic reactions are chemical reactions that release energy, usually in the form of heat, to their surroundings. They are characterized by a decrease in enthalpy (\(\Delta H < 0\)), indicating that the reactants have more stored energy than the products. In an exothermic reaction like the combustion of methane, the energy released occurs when the chemical bonds in the reactants break and new bonds form to create the products. The bond-breaking process absorbs energy, while bond-forming releases energy. If the energy released is more than the energy absorbed, the reaction is exothermic.
These reactions are often spontaneous and can be identified by a rise in temperature of the mixture or surrounding environment. An example of an everyday exothermic reaction is the burning of wood, which releases heat that we can feel—a similar process to the combustion happening with methane on a gas stove.
These reactions are often spontaneous and can be identified by a rise in temperature of the mixture or surrounding environment. An example of an everyday exothermic reaction is the burning of wood, which releases heat that we can feel—a similar process to the combustion happening with methane on a gas stove.
Combustion of Hydrocarbons
The combustion of hydrocarbons is a specific type of chemical reaction where a hydrocarbon reacts with oxygen to form carbon dioxide and water. Hydrocarbons are organic compounds composed of hydrogen and carbon, such as methane (\(\mathrm{CH}_{4}\)). During complete combustion, ample oxygen ensures that the hydrocarbon is entirely converted into \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2}\mathrm{O}\), releasing heat. Conversely, incomplete combustion occurs when oxygen is limited, resulting in the production of carbon monoxide (\(\mathrm{CO}\)) or even carbon soot.
Hydrocarbon combustion is a widely used chemical process for energy generation. Gasoline and natural gas are common fuels that undergo combustion. When methane combusts on a gas stove burner, its reaction with oxygen is an instance of hydrocarbon combustion that we use daily.
Hydrocarbon combustion is a widely used chemical process for energy generation. Gasoline and natural gas are common fuels that undergo combustion. When methane combusts on a gas stove burner, its reaction with oxygen is an instance of hydrocarbon combustion that we use daily.
Stoichiometry in Chemical Reactions
Stoichiometry refers to the quantitative relationship between reactants and products in a chemical reaction. It is based on the balanced chemical equation, which provides the molar ratio of the substances involved. By knowing the stoichiometry of a reaction, you can determine the amount of reactants needed to produce a certain amount of product or vice versa.
For example, the stoichiometry of the combustion of methane shows a 1:2 molar ratio of methane (\(\mathrm{CH}_{4}\)) to oxygen (\(\mathrm{O}_{2}\)). This indicates that for every one mole of methane, two moles of oxygen are required for complete combustion. This stoichiometric relationship also helps with calculations involving reaction yields, limits, and theoretical predictions of outcome amounts, making it a crucial aspect of chemical reaction planning and analysis.
For example, the stoichiometry of the combustion of methane shows a 1:2 molar ratio of methane (\(\mathrm{CH}_{4}\)) to oxygen (\(\mathrm{O}_{2}\)). This indicates that for every one mole of methane, two moles of oxygen are required for complete combustion. This stoichiometric relationship also helps with calculations involving reaction yields, limits, and theoretical predictions of outcome amounts, making it a crucial aspect of chemical reaction planning and analysis.