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Chapter 7: Q70E (page 400)

Question: Using the standard enthalpy of formation data in Appendix G, calculate the bond energy of the carbon-sulphur double bond in \({\rm{C}}{{\rm{S}}_{\rm{2}}}\).

Short Answer

Expert verified

Using the standard enthalpy of formation of \({\rm{C}}{{\rm{S}}_{\rm{2}}}{\rm{(g)}}\), the bond energy is determined as \({\rm{578}}{\rm{.7\;kJ}}\).

Step by step solution

01

Concept Introduction

Bond energy, also known as mean bond enthalpy or average bond enthalpy in chemistry, is a measure of the bond strength.It is the energy needed to dissociate the bonds into atoms.

02

Reactions and their Enthalpy

The reactions with their enthalpy values are 鈥�

\(\begin{array}{*{20}{l}}{{\rm{C}}{{\rm{S}}_{\rm{2}}}{\rm{(g)}} \to {\rm{C( graphite ) + 2\;S(s)}}}&{{\rm{\Delta H}}_{\rm{1}}^{\rm{^\circ }}{\rm{ = \Delta H}}_{{\rm{f}}\left( {{\rm{C}}{{\rm{S}}_{\rm{2}}}{\rm{(g)}}} \right)}^{\rm{^\circ }}}\\{{\rm{C(graphite)}} \to {\rm{C(g)}}}&{{\rm{\Delta H}}_{\rm{2}}^{\rm{^\circ }}{\rm{ = \Delta H}}_{{\rm{f(Cl)(g))}}}^{\rm{^\circ }}}\\{{\rm{2\;S(s)}} \to {\rm{2\;S(9)}}}&{{\rm{2\Delta H}}_{\rm{3}}^{\rm{^\circ }}{\rm{ = 2\Delta H}}_{{\rm{f(S(g))}}}^{\rm{^\circ }}}\end{array}\)

03

Bond Energy Calculation

The net reaction is 鈥�

\({\rm{C}}{{\rm{S}}_{\rm{2}}}{\rm{(g)}} \to {\rm{C(graphite) + 2\;S(g)}}\;\)

\(\begin{array}{c}{\rm{\Delta H}}_{{\rm{298}}}^{\rm{^\circ }}{\rm{ = \Delta }}{{\rm{H}}_{\rm{1}}}^{\rm{^\circ }}{\rm{ + \Delta H}}_{\rm{2}}^{\rm{^\circ }}{\rm{ + 2\Delta }}{{\rm{H}}_{\rm{3}}}^{\rm{^\circ }}\\{{\rm{D}}_{{\rm{C}}{{\rm{S}}_{\rm{2}}}}}{\rm{ = \Delta }}{{\rm{H}}^{\rm{^\circ }}}_{{\rm{298}}}{\rm{ = - \Delta }}{{\rm{H}}^{\rm{^\circ }}}_{{\rm{f}}\left( {{\rm{C}}{{\rm{S}}_{\rm{2}}}{\rm{(g)}}} \right)}{\rm{ + \Delta H}}_{{\rm{f(C(g))}}}^{\rm{^\circ }}{\rm{ + 2\Delta }}{{\rm{H}}^{\rm{^\circ }}}_{{\rm{f(S(g))}}}\end{array}\)

The bond energy is calculated as 鈥�

\(\begin{array}{c}{{\rm{D}}_{{\rm{C}}{{\rm{S}}_{\rm{2}}}}}{\rm{ = - 116}}{\rm{.9 + 716}}{\rm{.681 + 2(278}}{\rm{.81)}}\\{\rm{ = 1157}}{\rm{.4\;kJ}}{{\rm{D}}_{{\rm{C = S}}}}\\{\rm{ = }}\frac{{{\rm{1157}}{\rm{.4}}}}{{\rm{2}}}\\{\rm{ = 578}}{\rm{.7\;kJ}}\end{array}\)

Therefore, the value for bond energy is \({\rm{578}}{\rm{.7\;kJ}}\).

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Most popular questions from this chapter

Identify the electron pair geometry and the molecular structure of each of the following molecules:

  1. \({\rm{CNIO}}\) (N is the central atom)
  2. \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\)(C is the central atom)
  4. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SO}}\)(S is the central atom)
  5. \({\rm{S}}{{\rm{O}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)(S is the central atom)
  6. \({\rm{Xe}}{{\rm{O}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)(Xe is the central atom)
  7. \({\rm{ClOF}}_{\rm{2}}^{\rm{ + }}\)(Cl is the central atom)

Which compound in each of the following pairs has the larger lattice energy? Note: \({\rm{M}}{{\rm{g}}^{{\rm{2 + }}}}\) and \({\rm{L}}{{\rm{i}}^{\rm{ + }}}\) have similar radii; \({{\rm{O}}^{{\rm{2 - }}}}\) and \({{\rm{F}}^{\rm{ - }}}\) have similar radii. Explain your choices.

(a) \({\rm{MgO}}\) or \({\rm{MgSe}}\)

(b) \({\rm{LiF}}\) or \({\rm{MgO}}\)

(c) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{O}}\) or \({\rm{LiCl}}\)

(d) \({\rm{L}}{{\rm{i}}_{\rm{2}}}{\rm{Se}}\) or \({\rm{MgO}}\)

Determine the formal charge of each element in the following:

(a) \({{\rm{H}}_{\rm{3}}}{{\rm{O}}^{\rm{ + }}}\)

(b) \({\rm{SO}}_{\rm{4}}^{{\rm{2 - }}}\)

(c) \({\rm{N}}{{\rm{H}}_{\rm{3}}}\)

(d) \({\rm{O}}_{\rm{2}}^{{\rm{2 - }}}\)

(e) \({{\rm{H}}_{\rm{2}}}{{\rm{O}}_{\rm{2}}}\)

Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to explore real molecules. On the Real Molecules tab, select 鈥渕odel鈥� mode and S2O. What is the model bond angle? Explain whether the 鈥渞eal鈥� bond angle should be larger or smaller than the ideal model angle.

The lattice energy of \({\rm{LiF}}\) is \({\rm{1023 kJ/mol}}\), and the \({\rm{Li - F}}\) distance is \({\rm{200}}{\rm{.8 pm}}\). \({\rm{NaF}}\) crystallizes in the same structure as \({\rm{LiF}}\) but with a \({\rm{Na - F}}\) distance of \({\rm{231 pm}}\). Which of the following values most closely approximates the lattice energy of \({\rm{NaF}}\): \({\rm{510, 890, 1023, 1175,}}\) or \({\rm{4090 kJ/mol}}\)? Explain your choice.
See all solutions

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