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Chapter 8: Problem 20

What are the products of the complete combustion of a hydrocarbon?

Short Answer

Expert verified
The products of a complete combustion of a hydrocarbon are carbon dioxide (CO2) and water (H2O).

Step by step solution

01

Define Hydrocarbon

A hydrocarbon is an organic compound made up of hydrogen and carbon atoms. They can have different structures, including chains, branches, and rings.
02

Define Combustion

Combustion is a chemical reaction that occurs between a substance and an oxidizer, which in most cases is oxygen, and it typically releases heat and light.
03

Define Complete Combustion

Complete combustion happens when a hydrocarbon burns in plenty of oxygen. It produces carbon dioxide and water as products.
04

Write the General Chemical Equation for Complete Combustion

The general chemical equation for complete combustion is: \[ \text{Hydrocarbon} + \text{O}_{2} \rightarrow \text{CO}_{2} + \text{H}_{2}\text{O} \] This equation represents a simplified version of the combustion reaction, and the actual stoichiometry would depend on the specific hydrocarbon.

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Most popular questions from this chapter

Identify the type of reaction for each of the following. Then, predict products for the reaction, and balance the equation." reaction occurs, write "no reaction." $$ \begin{array}{l}{\text { a. water }+\text { lithium } \longrightarrow} \\\ {\text { b. silver nitrate + hydrochloric acid } \rightarrow} \\ {\text { c. hydrogen iodide } \rightarrow}\end{array} $$

Complete and balance the equation for the complete combustion of each of the following. $$ \begin{array}{ll}{\text { a. } C_{3} \mathrm{H}_{6}} & {\text { c. } C \mathrm{H}_{3} \mathrm{OH}} \\ {\text { b. } C_{5} \mathrm{H}_{12}} & {\text { d. } C_{12} \mathrm{H}_{22} \mathrm{O}_{11}}\end{array} $$

Write an unbalanced chemical equation for each of the following. $$\begin{array}{l}{\text { a. Aluminum reacts with oxygen to produce }} \\\ {\text { aluminum oxide. }} \\ {\text { b. Phosphoric acid, } \mathrm{H}_{3} \mathrm{PO}_{4} \text { , is produced }} \\ {\text { through the reaction between tetraphosphorus}} \\ {\text { decoxide and water. }}\end{array}$$

How does the process of balancing an equation illustrate the law of conservation of mass?

Use the activity series to predict whether the following reactions are possible. Explain your answers. $$\text {a}.\mathrm{Ni}(s)+\mathrm{MgSO}_{4}(a q) \longrightarrow{\mathrm{NiSO}_{4}(a q)+\mathrm{Mg}(s)}$$ $$\begin{array}{r}{\text { b. } 3 \mathrm{Mg}(s)+\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q) \longrightarrow} {3 \mathrm{MgSO}_{4}(a q)+2 \mathrm{Al}(s)}\end{array}$$ $$\text{c} \cdot \mathrm{Pb}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow{\mathrm{Pb}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2}(g)} $$
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