04. Bond Energy
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Thermodynamics

273041 What will be the enthalpy of formation of $\mathrm{NO}_2$ from the given bond dissociation enthalpy values? The bond dissociation enthalpy values for $\mathrm{O}_2, \mathrm{NO}$ and $\mathrm{NO}_2$ are as follows, $\mathrm{O}_{2(\mathrm{~g})}$ : $0 \mathrm{~kJ} / \mathrm{mol}, \mathrm{NO}_{(\mathrm{g})}: 90.25 \mathrm{~kJ} / \mathrm{mol}$ and $\mathrm{NO}_{2(\mathrm{~g})}: 33.18$ $\mathrm{kJ} / \mathrm{mol}$ respectively.

1 $+114.1 \mathrm{~kJ}$
2 $+52.7 \mathrm{~kJ}$
3 $-52.7 \mathrm{~kJ}$
4 $-114.1 \mathrm{~kJ}$
J and K CET-(2018)
Thermodynamics

273043 The dissociation energy of $\mathrm{CH}_4$ and $\mathrm{C}_2 \mathrm{H}_6$ to convert them into gaseous atoms are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

1 $130 \mathrm{kcal} / \mathrm{mol}$
2 $80 \mathrm{kcal} / \mathrm{mol}$
3 $180 \mathrm{kcal} / \mathrm{mol}$
4 $260 \mathrm{kcal} / \mathrm{mol}$
J and K CET-(1998)
Thermodynamics

273044 What is the $\triangle H$ of the reaction

The average bond energies of $\mathrm{C}-\mathrm{Cl}$ bond and $\mathrm{C}-\mathrm{H}$ bond are $416 \mathrm{~kJ}$ and $325 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively.

1 $1482 \mathrm{~kJ}$
2 $1482 \mathrm{~J}$
3 $1492 \mathrm{~kJ}$
4 $1492 \mathrm{~J}$
JIPMER-2010
Thermodynamics

273046 Identify the equation in which change in enthalpy is equal to change in internal energy

1 $2 \mathrm{H}_2 \mathrm{O}_2(l) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(l)+\mathrm{O}_2(\mathrm{~g})$
2 $\mathrm{C}(\mathrm{S})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})$
$\mathrm{n}_{\mathrm{g}}=1-1=0$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Rightarrow \quad \Delta \mathrm{H}=\Delta \mathrm{U}$
3 $\quad \mathrm{PCl}_5(\mathrm{~g}) \rightarrow \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}}=2-1=1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\mathrm{RT}$
4 $\quad \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}=2-3=-1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}-\mathrm{RT}$
MHT CET-02.05.2019
NEET DIGITAL LIBRARY
Thermodynamics

273041 What will be the enthalpy of formation of $\mathrm{NO}_2$ from the given bond dissociation enthalpy values? The bond dissociation enthalpy values for $\mathrm{O}_2, \mathrm{NO}$ and $\mathrm{NO}_2$ are as follows, $\mathrm{O}_{2(\mathrm{~g})}$ : $0 \mathrm{~kJ} / \mathrm{mol}, \mathrm{NO}_{(\mathrm{g})}: 90.25 \mathrm{~kJ} / \mathrm{mol}$ and $\mathrm{NO}_{2(\mathrm{~g})}: 33.18$ $\mathrm{kJ} / \mathrm{mol}$ respectively.

1 $+114.1 \mathrm{~kJ}$
2 $+52.7 \mathrm{~kJ}$
3 $-52.7 \mathrm{~kJ}$
4 $-114.1 \mathrm{~kJ}$
J and K CET-(2018)
Thermodynamics

273043 The dissociation energy of $\mathrm{CH}_4$ and $\mathrm{C}_2 \mathrm{H}_6$ to convert them into gaseous atoms are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

1 $130 \mathrm{kcal} / \mathrm{mol}$
2 $80 \mathrm{kcal} / \mathrm{mol}$
3 $180 \mathrm{kcal} / \mathrm{mol}$
4 $260 \mathrm{kcal} / \mathrm{mol}$
J and K CET-(1998)
Thermodynamics

273044 What is the $\triangle H$ of the reaction

The average bond energies of $\mathrm{C}-\mathrm{Cl}$ bond and $\mathrm{C}-\mathrm{H}$ bond are $416 \mathrm{~kJ}$ and $325 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively.

1 $1482 \mathrm{~kJ}$
2 $1482 \mathrm{~J}$
3 $1492 \mathrm{~kJ}$
4 $1492 \mathrm{~J}$
JIPMER-2010
Thermodynamics

273046 Identify the equation in which change in enthalpy is equal to change in internal energy

1 $2 \mathrm{H}_2 \mathrm{O}_2(l) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(l)+\mathrm{O}_2(\mathrm{~g})$
2 $\mathrm{C}(\mathrm{S})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})$
$\mathrm{n}_{\mathrm{g}}=1-1=0$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Rightarrow \quad \Delta \mathrm{H}=\Delta \mathrm{U}$
3 $\quad \mathrm{PCl}_5(\mathrm{~g}) \rightarrow \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}}=2-1=1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\mathrm{RT}$
4 $\quad \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}=2-3=-1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}-\mathrm{RT}$
MHT CET-02.05.2019
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Thermodynamics

273041 What will be the enthalpy of formation of $\mathrm{NO}_2$ from the given bond dissociation enthalpy values? The bond dissociation enthalpy values for $\mathrm{O}_2, \mathrm{NO}$ and $\mathrm{NO}_2$ are as follows, $\mathrm{O}_{2(\mathrm{~g})}$ : $0 \mathrm{~kJ} / \mathrm{mol}, \mathrm{NO}_{(\mathrm{g})}: 90.25 \mathrm{~kJ} / \mathrm{mol}$ and $\mathrm{NO}_{2(\mathrm{~g})}: 33.18$ $\mathrm{kJ} / \mathrm{mol}$ respectively.

1 $+114.1 \mathrm{~kJ}$
2 $+52.7 \mathrm{~kJ}$
3 $-52.7 \mathrm{~kJ}$
4 $-114.1 \mathrm{~kJ}$
J and K CET-(2018)
Thermodynamics

273043 The dissociation energy of $\mathrm{CH}_4$ and $\mathrm{C}_2 \mathrm{H}_6$ to convert them into gaseous atoms are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

1 $130 \mathrm{kcal} / \mathrm{mol}$
2 $80 \mathrm{kcal} / \mathrm{mol}$
3 $180 \mathrm{kcal} / \mathrm{mol}$
4 $260 \mathrm{kcal} / \mathrm{mol}$
J and K CET-(1998)
Thermodynamics

273044 What is the $\triangle H$ of the reaction

The average bond energies of $\mathrm{C}-\mathrm{Cl}$ bond and $\mathrm{C}-\mathrm{H}$ bond are $416 \mathrm{~kJ}$ and $325 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively.

1 $1482 \mathrm{~kJ}$
2 $1482 \mathrm{~J}$
3 $1492 \mathrm{~kJ}$
4 $1492 \mathrm{~J}$
JIPMER-2010
Thermodynamics

273046 Identify the equation in which change in enthalpy is equal to change in internal energy

1 $2 \mathrm{H}_2 \mathrm{O}_2(l) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(l)+\mathrm{O}_2(\mathrm{~g})$
2 $\mathrm{C}(\mathrm{S})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})$
$\mathrm{n}_{\mathrm{g}}=1-1=0$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Rightarrow \quad \Delta \mathrm{H}=\Delta \mathrm{U}$
3 $\quad \mathrm{PCl}_5(\mathrm{~g}) \rightarrow \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}}=2-1=1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\mathrm{RT}$
4 $\quad \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}=2-3=-1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}-\mathrm{RT}$
MHT CET-02.05.2019
For More Updates join with Us
NEET Test Series from KOTA - 10 Papers In MS WORD WhatsApp Here
Thermodynamics

273041 What will be the enthalpy of formation of $\mathrm{NO}_2$ from the given bond dissociation enthalpy values? The bond dissociation enthalpy values for $\mathrm{O}_2, \mathrm{NO}$ and $\mathrm{NO}_2$ are as follows, $\mathrm{O}_{2(\mathrm{~g})}$ : $0 \mathrm{~kJ} / \mathrm{mol}, \mathrm{NO}_{(\mathrm{g})}: 90.25 \mathrm{~kJ} / \mathrm{mol}$ and $\mathrm{NO}_{2(\mathrm{~g})}: 33.18$ $\mathrm{kJ} / \mathrm{mol}$ respectively.

1 $+114.1 \mathrm{~kJ}$
2 $+52.7 \mathrm{~kJ}$
3 $-52.7 \mathrm{~kJ}$
4 $-114.1 \mathrm{~kJ}$
J and K CET-(2018)
Thermodynamics

273043 The dissociation energy of $\mathrm{CH}_4$ and $\mathrm{C}_2 \mathrm{H}_6$ to convert them into gaseous atoms are 360 and $620 \mathrm{kcal} / \mathrm{mol}$ respectively. The bond energy of $\mathrm{C}-\mathrm{C}$ bond is

1 $130 \mathrm{kcal} / \mathrm{mol}$
2 $80 \mathrm{kcal} / \mathrm{mol}$
3 $180 \mathrm{kcal} / \mathrm{mol}$
4 $260 \mathrm{kcal} / \mathrm{mol}$
J and K CET-(1998)
Thermodynamics

273044 What is the $\triangle H$ of the reaction

The average bond energies of $\mathrm{C}-\mathrm{Cl}$ bond and $\mathrm{C}-\mathrm{H}$ bond are $416 \mathrm{~kJ}$ and $325 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively.

1 $1482 \mathrm{~kJ}$
2 $1482 \mathrm{~J}$
3 $1492 \mathrm{~kJ}$
4 $1492 \mathrm{~J}$
JIPMER-2010
Thermodynamics

273046 Identify the equation in which change in enthalpy is equal to change in internal energy

1 $2 \mathrm{H}_2 \mathrm{O}_2(l) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(l)+\mathrm{O}_2(\mathrm{~g})$
2 $\mathrm{C}(\mathrm{S})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})$
$\mathrm{n}_{\mathrm{g}}=1-1=0$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Rightarrow \quad \Delta \mathrm{H}=\Delta \mathrm{U}$
3 $\quad \mathrm{PCl}_5(\mathrm{~g}) \rightarrow \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}}=2-1=1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\mathrm{RT}$
4 $\quad \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$
$\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}=2-3=-1$
$\Delta \mathrm{H}=\Delta \mathrm{U}+\Delta \mathrm{n}_{\mathrm{g}} \mathrm{RT}$
$\Delta \mathrm{H}=\Delta \mathrm{U}-\mathrm{RT}$
MHT CET-02.05.2019