Using the data provided, calculate the multiple bond energy $(kJ\,mo{l^{ - 1}})$of a C&equiv;C bond in ${{\rm{C}}_2}{{\rm{H}}_2}.$ Given that the heat of formation of ${{\rm{C}}_2}{{\rm{H}}_2}$ is $225kJmo{l^{ - 1}}$ (take the bond energy of C─H bond as $350\,\,kJ\,\,mo{l^{ - 1}}.):$ $2{\rm{C}}\left( s \right) \to 2{\rm{C}}\left( {\rm{g}} \right)\Delta H = 1410\,\,{\rm{kJ\,\,mo}}{{\rm{l}}^{ - 1}}$ $2{\rm{C}}\left( s \right) \to 2{\rm{C}}\left( {\rm{g}} \right)\Delta H = 1410\,\,{\rm{kJ\,\,mo}}{{\rm{l}}^{ - 1}}$ ${{\rm{H}}_2}\left( {\rm{g}} \right) \to 2{\rm{H}}\left( {\rm{g}} \right)\Delta H = 330\,\,{\rm{kJ\,\,mo}}{{\rm{l}}^{ - 1}}$

JEE CHEMISTRY MCQ: THERMODYNAMICS

1 Hard

1 of 1

Application +4 | -1

Using the data provided, calculate the multiple bond energy

(kJ\,mo{l^{ - 1}})

of a C&equiv;C bond in

{\mathrm{C}_2}{\mathrm{H}_2}.

Given that the heat of formation of

{\mathrm{C}_2}{\mathrm{H}_2}

225kJmo{l^{ - 1}}

(take the bond energy of C─H bond as

350\,\,kJ\,\,mo{l^{ - 1}}.):

2\mathrm{C}\left( s \right) \to 2\mathrm{C}\left( \mathrm{g} \right)\Delta H = 1410\,\,\mathrm{kJ\,\,mo}{\mathrm{l}^{ - 1}}

2\mathrm{C}\left( s \right) \to 2\mathrm{C}\left( \mathrm{g} \right)\Delta H = 1410\,\,\mathrm{kJ\,\,mo}{\mathrm{l}^{ - 1}}

{\mathrm{H}_2}\left( \mathrm{g} \right) \to 2\mathrm{H}\left( \mathrm{g} \right)\Delta H = 330\,\,\mathrm{kJ\,\,mo}{\mathrm{l}^{ - 1}}

View answer and explanation

Correct option: D

815

The correct answer is D (815) because it's the calculated C≡C bond energy using the given heat of formation and bond energies.

Practice All Chapter MCQs →

\ \mathrm{C}(\mathrm{s})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})-\mathrm{CO}(\mathrm{g}), \Delta \mathrm{H}_1=\mathrm{a}

\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g})-\mathrm{CO}_2(\mathrm{~g}), \Delta \mathrm{H}_2=\mathrm{b}

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{~g})-2 \mathrm{CO}(\mathrm{g}) ; \Delta \mathrm{H}_3=\mathrm{c}

0.18 \mathrm{~g}

4 \mathrm{~K}.

\left(\Delta_{\mathrm{C}} \text{H}^{\circ}=-2.8\times 10^6 \mathrm{~J} / \mathrm{mol} \text{ glucose}\right)

{CsI}

{CsCl}

{CsCl}

{Cs} I

\begin{array}{cccccccccccccccccccc} {}&{\Delta H(KJ/mol)} \\ {1/2A \to B}&{ + 150} \\ {3B \to 2C + D}&{ - 125} \\ {E + A \to 2D}&{ + 350} \end{array}

{B}+{D} \rightarrow {E}+2 {C}, \Delta {H}

\Delta H

\Delta u

\mathrm{C}{\mathrm{H}_4}\left( \mathrm{g} \right) + 2{\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + {\mathrm{H}_2}\mathrm{O}\left( l \right);\Delta H = - 890.3\mathrm{kJ}