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Chapter 7: Q68E (page 400)

Question: How does the bond energy of \({\rm{HCl(g)}}\) differ from the standard enthalpy of formation of \({\rm{HCl(g)}}\)?

Short Answer

Expert verified

The bond energy differs from standard enthalpy for \({\rm{HCl}}\) as bond energy and enthalpy breaks \({\rm{HCl}}\) into \({\rm{H}}\) and \({\rm{Cl}}\) atoms and, \({{\rm{H}}_{\rm{2}}}\) and \({\rm{Cl}}\), molecules respectively.

Step by step solution

01

Concept Introduction

Bond energy gives the measure of the strength of bond in a chemical reaction.

02

Difference in bond energy and standard enthalpy of Hydrochloric Acid

The enthalpy change is when a mole of a substance is created from its elements in their standard states under standard conditions is called enthalpy of formation.

\({\rm{HCl(g)}} \to {{\rm{H}}_{\rm{2}}}{\rm{(g) + Cl(g)}}\)

Bond enthalpy is quite different and is a measure of the strength of an individual bond.

\({\rm{HCl(g)}} \to {\rm{H(g) + Cl(g)}}\)

Bond energy involves breaking of \({\rm{HCl}}\) molecule into \({\rm{H}}\) and \({\rm{Cl}}\) atoms whereas enthalpy of formation involves making of \({\rm{HCl}}\) from \({{\rm{H}}_{\rm{2}}}\) and \({\rm{Cl}}\), molecules.

Therefore, bond energy of \({\rm{HCl}}\) differ from the standard enthalpy of formation of \({\rm{HCl}}\).

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Most popular questions from this chapter

Correct the following statement: “The bonds in solid\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are ionic; the bond in a\({\text{HCl}}\)molecule is covalent. Thus, all of the valence electrons in\({\text{PbC}}{{\text{I}}_{\text{2}}}\)are located on the\({\text{C}}{{\text{I}}^{\text{ - }}}\)ions, and all of the valence electrons in a\({\text{HCl}}\)molecule are shared between the\({\text{H}}\)and\({\text{CI}}\)atoms.”

The reaction of a metal, \({\rm{M}}\), with a halogen, \({{\rm{X}}_{\rm{2}}}\), proceeds by an exothermic reaction as indicated by this equation: \({\rm{M(s) + }}{{\rm{X}}_{\rm{2}}}{\rm{(g)}} \to {\rm{M}}{{\rm{X}}_{\rm{2}}}{\rm{(s)}}\). For each of the following, indicate which option will make the reaction more exothermic. Explain your answers.

(a) a large radius vs. a small radius for \({{\rm{M}}^{{\rm{ + 2}}}}\)

(b) a high ionization energy vs. a low ionization energy for \({\rm{M}}\)

(c) an increasing bond energy for the halogen

(d) a decreasing electron affinity for the halogen

(e) an increasing size of the anion formed by the halogen

Question: Which bond in each of the following pairs of bonds is the strongest?

(a) \({\rm{C - C}}\) or \({\rm{C = C}}\)

(b) \({\rm{C - N}}\) or \({\rm{C}} \equiv {\rm{N}}\)

(c) \({\rm{C}} \equiv {\rm{O}}\) or \({\rm{C = O}}\)

(d) \({\rm{H - F}}\) or \({\rm{H - Cl}}\)

(e) \({\rm{C - H}}\) or \({\rm{O - H}}\)

(f) \({\rm{C - N}}\) or \({\rm{C - O}}\)

A compound with a molar mass of about \({\rm{42\;g/mol}}\) contains \({\rm{85}}{\rm{.7\% }}\)carbon and \({\rm{14}}{\rm{.3\% }}\) hydrogen. What is its molecular structure?

Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:

(a)\({\rm{S}}{{\rm{F}}_{\rm{6}}}\)

(b)\({\rm{PC}}{{\rm{l}}_{\rm{5}}}\)

(c)\({\rm{Be}}{{\rm{H}}_{\rm{2}}}\)

(d) \({\rm{CH}}_{\rm{3}}^{\rm{ + }}\)
See all solutions

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