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Chapter 6: Problem 14

Liquefied propane gas is often used for cooking in suburban areas away from natural gas lines. Propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) burns in oxygen gas, producing carbon dioxide gas, water vapor, and heat. Write the unbalanced chemical equation for this process.

Short Answer

Expert verified
The unbalanced chemical equation for the combustion of propane (\(\mathrm{C_3H_8}\)) in oxygen gas (\(\mathrm{O_2}\)) is: \(\mathrm{C_3H_8 + O_2 \rightarrow CO_2 + H_2O + heat}\)

Step by step solution

01

Write the chemical formulas of reactants

Start by writing the chemical formulas for propane and oxygen gas, which are the reactants in this process. Propane has the formula C₃H₈, and oxygen gas exists as a diatomic molecule O₂.
02

Write the chemical formulas of products

Now write the chemical formulas for the products of this combustion reaction, which are carbon dioxide gas (CO₂), water vapor (H₂O), and heat.
03

Combine reactants and products

Now that we have the chemical formulas for reactants and products, we can combine them to create the unbalanced equation\: C₃H₈ + O₂ → CO₂ + H₂O +heat
04

Unbalanced equation

The unbalanced chemical equation for the combustion of propane in oxygen gas is as follows: C₃H₈ + O₂ → CO₂ + H₂O + heat

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Reactions
Chemical reactions involve the transformation of one or more substances into different substances through the breaking and forming of chemical bonds. A classic example of a chemical reaction is the combustion of propane, also known as an exothermic reaction because it releases energy in the form of heat. In this particular reaction, propane (\text{C\(_3\)H\(_8\)}) reacts with oxygen (\text{O\(_2\)}) from the air to form carbon dioxide (\text{CO\(_2\)}) and water vapor (\text{H\(_2\)O}), releasing heat as a byproduct. Such reactions are fundamental in various applications, from residential heating to industrial processes. Understanding the reactants and products involved gives us insight into the conservation of mass and energy, as well as the quantitative relationships between materials before and after the chemical change.

Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It is based on the balancing of equations to ensure that the number of atoms for each element is conserved throughout the reaction. The stoichiometry of the combustion of propane requires knowing the coefficients that balance the molecules of propane and oxygen with the molecules of carbon dioxide and water formed. This mathematical approach allows us to predict the amounts of reactants needed and products formed. For example, in the combustion process, understanding stoichiometry enables us to calculate the amount of oxygen required to burn a certain volume of propane completely or the quantity of carbon dioxide produced, which has important implications for energy efficiency and environmental concerns.

Balancing Chemical Equations
Balancing chemical equations is crucial for correctly representing the conservation of mass in a chemical reaction. An equation must have the same number of each type of atom on both sides of the reaction arrow. To achieve this, coefficients are placed in front of the chemical formulas to indicate the number of each type of molecule involved. For instance, the incomplete combustion of propane starts with a simple representation: \text{C\(_3\)H\(_8\) + O\(_2\) \rightarrow CO\(_2\) + H\(_2\)O + heat}. Through the process of balancing the equation, we adjust the coefficients to ensure that the same number of carbon, hydrogen, and oxygen atoms are present on both the reactant and product sides. This is a foundational skill in chemistry because it allows us to use the reaction equation to carry out stoichiometric calculations, which are key for everything from cooking with gas to industrial-scale chemical production and reducing pollutants in emissions.

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Most popular questions from this chapter

Pennies in the United States now consist of a zinc disk that is coated with a thin layer of copper. If a penny is scratched and then soaked in hydrochloric acid, it is possible to dissolve the zinc disk, leaving only a thin, hollow shell of copper. Write an unbalanced chemical equation to illustrate the reaction of zinc metal with hydrochloric acid, which produces dissolved zinc chloride and evolves gaseous hydrogen.

You have probably had the unpleasant experience of discovering that a flashlight battery has gotten old and begun to leak. Is there evidence that this change is due to a chemical reaction?

Glass is a mixture of several compounds, but a major constituent of most glass is calcium silicate, Ca\(\mathrm{SiO}_{3} .\) Glass can be etched by treatment with hydrogen fluoride: HF attacks the calcium silicate of the glass, producing gaseous and water-soluble products (which can be removed by washing the glass). For example, the volumetric glassware in chemistry laboratories is often graduated by using this process. Balance the following equation for the reaction of hydrogen fluoride with calcium silicate.$$\mathrm{CaSiO}_{3}(s)+\mathrm{HF}(g) \rightarrow \mathrm{CaF}_{2}(a q)+\mathrm{SiF}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(l).$$

If you have had a clogged sink drain at your home, you have undoubtedly tried using a commercial drain cleaner to dissolve the clog. What evidence is there that such drain cleaners work by chemical reaction?

Balance each of the following chemical equations. a. \(\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{KOH}(a q)+\mathrm{O}_{2}(g)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)\) b. \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) c. \(\mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}(g)+\mathrm{H}_{2} \mathrm{O}(g)\) d. \(\mathrm{PCl}_{5}(l)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{HCl}(g)\) e. \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) f. \(\operatorname{CaO}(s)+\mathrm{C}(s) \rightarrow \mathrm{CaC}_{2}(s)+\mathrm{CO}_{2}(g)\) g. \(\operatorname{MoS}_{2}(s)+\mathrm{O}_{2}(g) \rightarrow \operatorname{MoO}_{3}(s)+\mathrm{SO}_{2}(g)\)h. \(\operatorname{Fe} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightarrow \mathrm{Fe}\left(\mathrm{HCO}_{3}\right)_{2}(a q)\)
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