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Chapter 7: Q35 E (page 395)

Methanol,\({{\text{H}}_{\text{3}}}{\text{COH}}\), is used as the fuel in some race cars. Ethanol,\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH}}\), is used extensively as motor fuel in Brazil. Both methanol and ethanol produce\({\text{C}}{{\text{O}}_{\text{2}}}\)and\({{\text{H}}_{\text{2}}}{\text{O}}\)when they burn. Write the chemical equations for these combustion reactions using Lewis structures instead of chemical formulas.

Short Answer

Expert verified

The combustion reaction using the Lewis structure for \({\text{C}}{{\text{H}}_{\text{3}}}{\text{OH }}\) is

The combustion reaction using the Lewis structure for \({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH }}\) is:


Step by step solution

01

Define Chemical Bonding

A chemical bond is a long-term inducement between atoms, ions, or molecules that permits chemical compounds to develop.

02

Writing the combustion reaction

The combustion reaction for \({\text{C}}{{\text{H}}_{\text{3}}}{\text{OH }}\) is

The combustion reaction for \({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH }}\)

Therefore, the reactions are

\({\text{C}}{{\text{H}}_{\text{3}}}{\text{OH }}\)-

\({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{5}}}{\text{OH }}\)-

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Most popular questions from this chapter

From its position in the periodic table, determine which atom in each pair is more electronegative: (a)\({\rm{Br or Cl}}\)(b)\({\rm{N or O}}\)(c)\({\rm{S or O}}\)(d)\({\rm{P or S}}\)(e)\({\rm{Si or N}}\)(f)\({\rm{Ba or P}}\)(g)\({\rm{N or K}}\).

Many monatomic ions are found in seawater, including the ions formed from the following list of elements. Write the Lewis symbols for the monatomic ions formed from the following elements: (a)\({\rm{CI}}\)(b)\({\rm{Na}}\)(c)\({\rm{Mg}}\)(d)\({\rm{Ca}}\)(e)\({\rm{K}}\)(f)\({\rm{Br}}\)(g)\({\rm{Sr}}\)(h)\({\rm{F}}\).

Question: Using the bond energies in Table \({\rm{7}}{\rm{.2}}\), determine the approximate enthalpy change for each of the following reactions:

(a) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{(g) + 3}}{{\rm{F}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2Cl}}{{\rm{F}}_{\rm{3}}}{\rm{(g)}}\)

(b) \({{\rm{H}}_{\rm{2}}}{\rm{C = C}}{{\rm{H}}_{\rm{2}}}{\rm{(g) + }}{{\rm{H}}_{\rm{2}}}{\rm{(g)}} \to {{\rm{H}}_{\rm{3}}}{\rm{CC}}{{\rm{H}}_{\rm{3}}}{\rm{(g)}}\)

(c) \({\rm{2}}{{\rm{C}}_{\rm{2}}}{{\rm{H}}_{\rm{6}}}{\rm{(g) + 7}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{4C}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + 6}}{{\rm{H}}_{\rm{2}}}{\rm{O(g)}}\)

Iron(\({\rm{III}}\)) sulfate (\({\rm{F}}{{\rm{e}}_{\rm{2}}}{{\rm{(S}}{{\rm{O}}_{\rm{4}}}{\rm{)}}_{\rm{3}}}\)) is composed of \({\rm{F}}{{\rm{e}}^{{\rm{3 + }}}}\) and \({\rm{S}}{{\rm{O}}_{\rm{4}}}^{{\rm{2 - }}}\) ions. Explain why a sample of iron(\({\rm{III}}\)) sulfate is uncharged.

Question: Using the standard enthalpy of formation data in Appendix G, determine which bond is stronger: the \({\rm{S - F}}\) bond in \({\rm{S}}{{\rm{F}}_{\rm{4}}}{\rm{(g)}}\) or in \({\rm{S}}{{\rm{F}}_{\rm{6}}}{\rm{(g)}}\)?
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