Standard enthalpy of combustion of $C H_{4}$ is $- 890 k J m o l^{- 1}$ and standard enthalpy of vaporisation of water is 40.5 kJ $m o l^{- 1}$ . Calculate the enthalpy change for the reaction :
$C H_{4 (g)} + 2 O_{2 (g)} \to C O_{2 (g)} + 2 H_{2} O_{(g)}$

Q. Bond dissociation enthalpies of

H_{2} (g) a n d N_{2} (g)

are

436.0 k J m o l^{- 1}

and

941.3 k J m o l^{- 1}

respectively. Enthalpy of formation of

N H_{3}

(g) is

- 46.0 k J m o l^{- 1}

. What is the enthalpy of atomization of

N H_{3}

The standard enthalpy of formation of $N H_{3}$ is $46.0 k J m o l^{- 1}$ . If the enthalpy of formation of $H_{2}$ from its atom is $- 436 k J m o l^{- 1}$ and that of $N_{2}$ is $- 712 k J m o l^{- 1}$ , the average bond enthalpy of $N - H$ bond in $N H_{3}$ is

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The standard enthalpy of formation of H2O(l) and Fe2O3(s) are respectively −286 kJ mol−1 and −824 kJ mol−1. What is the standard enthalpy change for the following reaction?Fe2O3(s)+3H2(g)⟶3H2O(l)+2Fe(s)

The standard enthalpy of formation of $H_{2} O (l)$ and ${F e}_{2} O_{3} (s)$ are respectively $- 286$ $k J$ ${m o l}^{- 1}$ and $- 824$ $k J$ ${m o l}^{- 1}$ . What is the standard enthalpy change for the following reaction?

${F e}_{2} O_{3} (s) + 3 H_{2} (g) ⟶ 3 H_{2} O (l) + 2 F e (s)$