(D) The bond dissociation energy (or bond energy) is defined as the energy required to break one mole of bonds in a gaseous molecule to produce gaseou

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$HCl_{(g)} \rightarrow H_{(g)} + Cl_{(g)}$

(D) The bond dissociation energy (or bond energy) is defined as the energy required to break one mole of bonds in a gaseous molecule to produce gaseous atoms.For $HCl_{(g)}$,the reaction representing the breaking of the $H-Cl$ bond into its constituent gaseous atoms is:$HCl_{(g)} \rightarrow H_{(g)} + Cl_{(g)}$Therefore,the correct option is $D$.

Class 11 Chemistry Thermodynamics Heat of reaction, Bond energy and Hess law

Easy

For which of the following reactions does the heat of reaction represent the bond energy of $HCl$?

A
$HCl_{(g)} \rightarrow H^{+}_{(g)} + Cl^{-}_{(g)}$
B
$HCl_{(g)} \rightarrow \frac{1}{2}H_{2(g)} + \frac{1}{2}Cl_{2(g)}$
C
$2HCl_{(g)} \rightarrow H_{2(g)} + Cl_{2(g)}$
D
$HCl_{(g)} \rightarrow H_{(g)} + Cl_{(g)}$

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Thermodynamics

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Heat of reaction, Bond energy and Hess law

The heat of combustion of ethanol into carbon dioxide and water is $-327 \ kcal$ at constant pressure. The heat evolved (in $cal$) at constant volume and $27^{\circ} C$ (assuming all gases behave ideally) is $\left( R = 2 \ cal \ mol^{-1} \ K^{-1} \right)$

DifficultJEE MAIN 2020

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The enthalpy of formation of $NH_3$ is $-46 \ kJ \ mol^{-1}$. The enthalpy change for the reaction $2 NH_{3(g)} \longrightarrow N_{2(g)} + 3 H_{2(g)}$ is

EasyKCET 2009

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In the reaction: $H_2 + Cl_2 \to 2HCl, \Delta H = -194 \ kJ$. The heat of formation of $HCl$ is ........ $kJ$.

Medium

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What is the standard enthalpy of reaction (in $kJ$) when two moles of $Fe_2O_{3(s)}$ react with $H_2$ gas to give $Fe$ metal? $\Delta H_f^{\circ}$ of $Fe_2O_{3(s)}$ and $H_2O_{(l)}$ are $-824.2$ and $-285.83 \ kJ \ mol^{-1}$ respectively.

MediumTS EAMCET 2019

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Given the thermochemical reactions:
$C(\text{graphite}) + \frac{1}{2} O_{2(g)} \to CO_{(g)}; \Delta H = -110.5 \ kJ$
$CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}; \Delta H = -283.2 \ kJ$
Calculate the heat of reaction for $C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}$ in $kJ$.

Medium

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For which of the following reactions does the heat of reaction represent the bond energy of $HCl$?

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The heat of combustion of ethanol into carbon dioxide and water is $-327 \ kcal$ at constant pressure. The heat evolved (in $cal$) at constant volume and $27^{\circ} C$ (assuming all gases behave ideally) is $\left( R = 2 \ cal \ mol^{-1} \ K^{-1} \right)$

The enthalpy of formation of $NH_3$ is $-46 \ kJ \ mol^{-1}$. The enthalpy change for the reaction $2 NH_{3(g)} \longrightarrow N_{2(g)} + 3 H_{2(g)}$ is

In the reaction: $H_2 + Cl_2 \to 2HCl, \Delta H = -194 \ kJ$. The heat of formation of $HCl$ is ........ $kJ$.

What is the standard enthalpy of reaction (in $kJ$) when two moles of $Fe_2O_{3(s)}$ react with $H_2$ gas to give $Fe$ metal? $\Delta H_f^{\circ}$ of $Fe_2O_{3(s)}$ and $H_2O_{(l)}$ are $-824.2$ and $-285.83 \ kJ \ mol^{-1}$ respectively.

Given the thermochemical reactions: $C(\text{graphite}) + \frac{1}{2} O_{2(g)} \to CO_{(g)}; \Delta H = -110.5 \ kJ$ $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}; \Delta H = -283.2 \ kJ$ Calculate the heat of reaction for $C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}$ in $kJ$.

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Given the thermochemical reactions:
$C(\text{graphite}) + \frac{1}{2} O_{2(g)} \to CO_{(g)}; \Delta H = -110.5 \ kJ$
$CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}; \Delta H = -283.2 \ kJ$
Calculate the heat of reaction for $C(\text{graphite}) + O_{2(g)} \to CO_{2(g)}$ in $kJ$.