(D) The standard enthalpy of formation,$\Delta H_f^o$,is defined as the enthalpy change when $1 \ mol$ of a compound is formed from its constituent el

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$Xe_{(g)} + 2F_{2(g)} \to XeF_{4(s)}$

(D) The standard enthalpy of formation,$\Delta H_f^o$,is defined as the enthalpy change when $1 \ mol$ of a compound is formed from its constituent elements in their standard states.For option $D$,$Xe_{(g)}$ and $F_{2(g)}$ are the standard states of the elements at $298 \ K$ and $1 \ bar$ pressure.Since $1 \ mol$ of $XeF_{4(s)}$ is formed from its elements in their standard states,$\Delta H_{react}^o = \Delta H_f^o$ for $XeF_{4(s)}$.

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

Medium

For which one of the following equations is $\Delta H_{react}^o$ equal to $\Delta H_f^o$ for the product?

AIPMT 2003 All AIPMT

A
$2CO_{(g)} + O_{2(g)} \to 2CO_{2(g)}$
B
$N_{2(g)} + O_{3(g)} \to N_2O_{3(g)}$
C
$CH_{4(g)} + 2Cl_{2(g)} \to CH_2Cl_{2(l)} + 2HCl_{(g)}$
D
$Xe_{(g)} + 2F_{2(g)} \to XeF_{4(s)}$

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Heat of reaction, Bond energy and Hess law

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At $298 \, K$,the bond energies of $C-H, C-C, C=C$,and $H-H$ are $414, 347, 615$,and $435 \, kJ \, mol^{-1}$ respectively. What will be the enthalpy change for the reaction ${H_2}C=CH_{2(g)} + H_{2(g)} \to H_3C-CH_{3(g)}$ at $298 \, K$ in $kJ \, mol^{-1}$?

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The heat of atomisation of methane and ethane are $x \ kJ \ mol^{-1}$ and $y \ kJ \ mol^{-1}$ respectively. The longest wavelength $(\lambda)$ of light capable of breaking the $C-C$ bond can be expressed in $SI$ unit as :

DifficultJEE MAIN 2026

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$H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}, \Delta H = -44 \ kcal$
$2Na_{(s)} + 2HCl_{(g)} \to 2NaCl_{(s)} + H_{2(g)}, \Delta H = -152 \ kcal$
For the reaction $Na_{(s)} + \frac{1}{2}Cl_{2(g)} \to NaCl_{(s)}, \Delta H = \dots \ kcal$

Medium

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The enthalpies of formation of $CO_{2(g)}$,$H_2O_{(g)}$,and $C_2H_{4(g)}$ are $-393.7$,$-241.8$,and $52.3 \ kJ \ mol^{-1}$ respectively. What will be the enthalpy of combustion of ethylene at $298 \ K$ and $1 \ atm$ pressure in $kJ \ mol^{-1}$?

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The enthalpy change for the reaction,$C_{2}H_{6(g)} \to 2C_{(g)} + 6H_{(g)}$ is $X \ kJ$. The bond energy of $C-H$ bond is :-

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For which one of the following equations is $\Delta H_{react}^o$ equal to $\Delta H_f^o$ for the product?

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At $298 \, K$,the bond energies of $C-H, C-C, C=C$,and $H-H$ are $414, 347, 615$,and $435 \, kJ \, mol^{-1}$ respectively. What will be the enthalpy change for the reaction ${H_2}C=CH_{2(g)} + H_{2(g)} \to H_3C-CH_{3(g)}$ at $298 \, K$ in $kJ \, mol^{-1}$?

The heat of atomisation of methane and ethane are $x \ kJ \ mol^{-1}$ and $y \ kJ \ mol^{-1}$ respectively. The longest wavelength $(\lambda)$ of light capable of breaking the $C-C$ bond can be expressed in $SI$ unit as :

$H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}, \Delta H = -44 \ kcal$$2Na_{(s)} + 2HCl_{(g)} \to 2NaCl_{(s)} + H_{2(g)}, \Delta H = -152 \ kcal$For the reaction $Na_{(s)} + \frac{1}{2}Cl_{2(g)} \to NaCl_{(s)}, \Delta H = \dots \ kcal$

The enthalpies of formation of $CO_{2(g)}$,$H_2O_{(g)}$,and $C_2H_{4(g)}$ are $-393.7$,$-241.8$,and $52.3 \ kJ \ mol^{-1}$ respectively. What will be the enthalpy of combustion of ethylene at $298 \ K$ and $1 \ atm$ pressure in $kJ \ mol^{-1}$?

The enthalpy change for the reaction,$C_{2}H_{6(g)} \to 2C_{(g)} + 6H_{(g)}$ is $X \ kJ$. The bond energy of $C-H$ bond is :-

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$H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}, \Delta H = -44 \ kcal$
$2Na_{(s)} + 2HCl_{(g)} \to 2NaCl_{(s)} + H_{2(g)}, \Delta H = -152 \ kcal$
For the reaction $Na_{(s)} + \frac{1}{2}Cl_{2(g)} \to NaCl_{(s)}, \Delta H = \dots \ kcal$