369526 Bond dissociation enthalpy of \(\mathrm{\mathrm{H}_{2}, \mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{HCl}}\) are 434, 242 and \(\mathrm{431 \mathrm{~kJ} \mathrm{~mol}^{-1}}\) respectively. Enthalpy of formation of \(\mathrm{\mathrm{HCl}}\) is

369527 If at \(298 \mathrm{~K}\), the bond energies of \(\mathrm{C}-\mathrm{H}, \mathrm{C}-\mathrm{C}, \mathrm{C}=\mathrm{C}\) and \(\mathrm{H}-\mathrm{H}\) bonds are respectively \(414,347,615\) and \(435 \mathrm{~kJ} \mathrm{~mol}^{-1}\), the value of enthalpy change for the reaction;
\(\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}(\mathrm{~g})\) at 298K, will be

369528 Given that, for the reaction, \(\dfrac{1}{2} \mathrm{H}_{2}+\dfrac{1}{2} \mathrm{Cl}_{2} \rightarrow \mathrm{HCl}\)
\[\begin{array}{l}
{\rm{\Delta }}{{\rm{H}}_{\rm{f}}}{\rm{(HCl}}) = - 93\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{{\rm{H}}_{\rm{2}}}} \right) = 434\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right) = 242\;{\rm{kJ}}/{\rm{mol}}
\end{array}\]
The bond dissociation energy of \(\mathrm{HCl}\) is.

369529 What is standard \(\mathrm{\mathrm{N} \equiv \mathrm{N}}\) bond enthalpy from following reaction,
\(\mathrm{\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g}) ; \Delta \mathrm{H}^{\mathrm{o}}=-83 \mathrm{~kJ}}\)
\(\left( {B \cdot E \cdot ({\rm{H - H}}){\rm{ = 435}}\;{\rm{kJ}};B \cdot E \cdot ({\rm{N - H}}){\rm{ = 389}}\;{\rm{kJ}}} \right)\)

369526 Bond dissociation enthalpy of \(\mathrm{\mathrm{H}_{2}, \mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{HCl}}\) are 434, 242 and \(\mathrm{431 \mathrm{~kJ} \mathrm{~mol}^{-1}}\) respectively. Enthalpy of formation of \(\mathrm{\mathrm{HCl}}\) is

369527 If at \(298 \mathrm{~K}\), the bond energies of \(\mathrm{C}-\mathrm{H}, \mathrm{C}-\mathrm{C}, \mathrm{C}=\mathrm{C}\) and \(\mathrm{H}-\mathrm{H}\) bonds are respectively \(414,347,615\) and \(435 \mathrm{~kJ} \mathrm{~mol}^{-1}\), the value of enthalpy change for the reaction;
\(\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}(\mathrm{~g})\) at 298K, will be

369528 Given that, for the reaction, \(\dfrac{1}{2} \mathrm{H}_{2}+\dfrac{1}{2} \mathrm{Cl}_{2} \rightarrow \mathrm{HCl}\)
\[\begin{array}{l}
{\rm{\Delta }}{{\rm{H}}_{\rm{f}}}{\rm{(HCl}}) = - 93\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{{\rm{H}}_{\rm{2}}}} \right) = 434\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right) = 242\;{\rm{kJ}}/{\rm{mol}}
\end{array}\]
The bond dissociation energy of \(\mathrm{HCl}\) is.

369529 What is standard \(\mathrm{\mathrm{N} \equiv \mathrm{N}}\) bond enthalpy from following reaction,
\(\mathrm{\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g}) ; \Delta \mathrm{H}^{\mathrm{o}}=-83 \mathrm{~kJ}}\)
\(\left( {B \cdot E \cdot ({\rm{H - H}}){\rm{ = 435}}\;{\rm{kJ}};B \cdot E \cdot ({\rm{N - H}}){\rm{ = 389}}\;{\rm{kJ}}} \right)\)

369526 Bond dissociation enthalpy of \(\mathrm{\mathrm{H}_{2}, \mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{HCl}}\) are 434, 242 and \(\mathrm{431 \mathrm{~kJ} \mathrm{~mol}^{-1}}\) respectively. Enthalpy of formation of \(\mathrm{\mathrm{HCl}}\) is

369527 If at \(298 \mathrm{~K}\), the bond energies of \(\mathrm{C}-\mathrm{H}, \mathrm{C}-\mathrm{C}, \mathrm{C}=\mathrm{C}\) and \(\mathrm{H}-\mathrm{H}\) bonds are respectively \(414,347,615\) and \(435 \mathrm{~kJ} \mathrm{~mol}^{-1}\), the value of enthalpy change for the reaction;
\(\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}(\mathrm{~g})\) at 298K, will be

369528 Given that, for the reaction, \(\dfrac{1}{2} \mathrm{H}_{2}+\dfrac{1}{2} \mathrm{Cl}_{2} \rightarrow \mathrm{HCl}\)
\[\begin{array}{l}
{\rm{\Delta }}{{\rm{H}}_{\rm{f}}}{\rm{(HCl}}) = - 93\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{{\rm{H}}_{\rm{2}}}} \right) = 434\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right) = 242\;{\rm{kJ}}/{\rm{mol}}
\end{array}\]
The bond dissociation energy of \(\mathrm{HCl}\) is.

369529 What is standard \(\mathrm{\mathrm{N} \equiv \mathrm{N}}\) bond enthalpy from following reaction,
\(\mathrm{\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g}) ; \Delta \mathrm{H}^{\mathrm{o}}=-83 \mathrm{~kJ}}\)
\(\left( {B \cdot E \cdot ({\rm{H - H}}){\rm{ = 435}}\;{\rm{kJ}};B \cdot E \cdot ({\rm{N - H}}){\rm{ = 389}}\;{\rm{kJ}}} \right)\)

369526 Bond dissociation enthalpy of \(\mathrm{\mathrm{H}_{2}, \mathrm{Cl}_{2}}\) and \(\mathrm{\mathrm{HCl}}\) are 434, 242 and \(\mathrm{431 \mathrm{~kJ} \mathrm{~mol}^{-1}}\) respectively. Enthalpy of formation of \(\mathrm{\mathrm{HCl}}\) is

369527 If at \(298 \mathrm{~K}\), the bond energies of \(\mathrm{C}-\mathrm{H}, \mathrm{C}-\mathrm{C}, \mathrm{C}=\mathrm{C}\) and \(\mathrm{H}-\mathrm{H}\) bonds are respectively \(414,347,615\) and \(435 \mathrm{~kJ} \mathrm{~mol}^{-1}\), the value of enthalpy change for the reaction;
\(\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}_{2}+\mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3}(\mathrm{~g})\) at 298K, will be

369528 Given that, for the reaction, \(\dfrac{1}{2} \mathrm{H}_{2}+\dfrac{1}{2} \mathrm{Cl}_{2} \rightarrow \mathrm{HCl}\)
\[\begin{array}{l}
{\rm{\Delta }}{{\rm{H}}_{\rm{f}}}{\rm{(HCl}}) = - 93\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{{\rm{H}}_{\rm{2}}}} \right) = 434\;{\rm{kJ}}/{\rm{mol}}\\
{\rm{BE}}\left( {{\rm{C}}{{\rm{l}}_{\rm{2}}}} \right) = 242\;{\rm{kJ}}/{\rm{mol}}
\end{array}\]
The bond dissociation energy of \(\mathrm{HCl}\) is.

369529 What is standard \(\mathrm{\mathrm{N} \equiv \mathrm{N}}\) bond enthalpy from following reaction,
\(\mathrm{\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{~g}) ; \Delta \mathrm{H}^{\mathrm{o}}=-83 \mathrm{~kJ}}\)
\(\left( {B \cdot E \cdot ({\rm{H - H}}){\rm{ = 435}}\;{\rm{kJ}};B \cdot E \cdot ({\rm{N - H}}){\rm{ = 389}}\;{\rm{kJ}}} \right)\)