(A) The molar mass of $H_2$ is $2 \ g/mol$. Number of moles of $H_2$ in $4 \ g = \frac{4 \ g}{2 \ g/mol} = 2 \ mol$. Bond energy is defined as the ene

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(A) The molar mass of $H_2$ is $2 \ g/mol$. Number of moles of $H_2$ in $4 \ g = \frac{4 \ g}{2 \ g/mol} = 2 \ mol$. Bond energy is defined as the energy required to dissociate $1 \ mole$ of bonds. Bond energy of $H-H = \frac{\text{Total energy}}{\text{Number of moles}} = \frac{208 \ kcal}{2 \ mol} = 104 \ kcal/mol$.

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

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Energy required to dissociate $4 \ g$ of gaseous hydrogen into free gaseous atoms is $208 \ kcal$ at $25 \ ^oC$. The bond energy of $H-H$ bond will be

A
$104 \ kcal$
B
$10.4 \ kcal$
C
$1040 \ kcal$
D
$104 \ cal$

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Class 11

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Thermodynamics

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Heat of reaction, Bond energy and Hess law

Which of the following pairs has a heat of neutralisation equal to $13.7 \, Kcal$?

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The heat of solution of $Na_2SO_{4(s)}$ and $Na_2SO_4 \cdot 10H_2O_{(s)}$ are $-2.34 \ kJ \ mol^{-1}$ and $78.87 \ kJ \ mol^{-1}$ respectively. The heat of hydration of $Na_2SO_{4(s)}$ is:

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$C_{(diamond)} + O_2 \to CO_2; \Delta H = -395.3 \ kJ/mole$
$C_{(graphite)} + O_2 \to CO_2; \Delta H = -393.4 \ kJ/mole$
$C_{(graphite)} \to C_{(diamond)}; \Delta H = ?$

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What will be the heat of formation of methane,if the heat of combustion of carbon is $-x \ kJ$,heat of formation of water is $-y \ kJ$ and heat of combustion of methane is $z \ kJ$?

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The enthalpy of combustion of ${C_6H_6}_{(l)}$ is $-3250 \, kJ/mol$. When $0.39 \, g$ of benzene is burnt in excess of oxygen in an open vessel,the amount of heat evolved is:

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Energy required to dissociate $4 \ g$ of gaseous hydrogen into free gaseous atoms is $208 \ kcal$ at $25 \ ^oC$. The bond energy of $H-H$ bond will be

Similar Questions

Which of the following pairs has a heat of neutralisation equal to $13.7 \, Kcal$?

The heat of solution of $Na_2SO_{4(s)}$ and $Na_2SO_4 \cdot 10H_2O_{(s)}$ are $-2.34 \ kJ \ mol^{-1}$ and $78.87 \ kJ \ mol^{-1}$ respectively. The heat of hydration of $Na_2SO_{4(s)}$ is:

$C_{(diamond)} + O_2 \to CO_2; \Delta H = -395.3 \ kJ/mole$$C_{(graphite)} + O_2 \to CO_2; \Delta H = -393.4 \ kJ/mole$$C_{(graphite)} \to C_{(diamond)}; \Delta H = ?$

What will be the heat of formation of methane,if the heat of combustion of carbon is $-x \ kJ$,heat of formation of water is $-y \ kJ$ and heat of combustion of methane is $z \ kJ$?

The enthalpy of combustion of ${C_6H_6}_{(l)}$ is $-3250 \, kJ/mol$. When $0.39 \, g$ of benzene is burnt in excess of oxygen in an open vessel,the amount of heat evolved is:

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$C_{(diamond)} + O_2 \to CO_2; \Delta H = -395.3 \ kJ/mole$
$C_{(graphite)} + O_2 \to CO_2; \Delta H = -393.4 \ kJ/mole$
$C_{(graphite)} \to C_{(diamond)}; \Delta H = ?$