Which of the following statements is correct about the heat of combustion?
- AIt may be exothermic in some cases and endothermic in other cases.
- BIt is applicable to gaseous substances only.
- CIt is always an exothermic reaction.
- DIts value does not change with temperature.
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Similar Questions
Which of the following fuels will have the highest calorific value $(kJ/kg)$?
Easy
View SolutionGiven that $C + O_{2} \longrightarrow CO_{2} ; \Delta H^{\circ} = -x \ kJ$ and $2 CO + O_{2} \longrightarrow 2 CO_{2} ; \Delta H^{\circ} = -y \ kJ$. The heat of formation of carbon monoxide will be
MediumWBJEE 2014
View SolutionFind the standard enthalpy of formation of $SO_{3(g)}$ from the following reactions:
$S_{8(s)} + 8O_{2(g)} \to 8SO_{2(g)}$; $\Delta H_1 = -2775 \ kJ/mol$
$2SO_{2(g)} + O_{2(g)} \to 2SO_{3(g)}$; $\Delta H_2 = -198 \ kJ/mol$
$S_{8(s)} + 8O_{2(g)} \to 8SO_{2(g)}$; $\Delta H_1 = -2775 \ kJ/mol$
$2SO_{2(g)} + O_{2(g)} \to 2SO_{3(g)}$; $\Delta H_2 = -198 \ kJ/mol$
Medium
View SolutionIf the enthalpies of atomization of methane and ethane are respectively $320 \ cal$ and $360 \ cal$,then the bond energy of the $C-C$ bond is......$cal$.
Medium
View SolutionFrom the following bond energies:
$H-H$ bond energy $431.37 \text{ kJ mol}^{-1}$ $C=C$ bond energy $606.10 \text{ kJ mol}^{-1}$ $C-C$ bond energy $336.49 \text{ kJ mol}^{-1}$ $C-H$ bond energy $410.50 \text{ kJ mol}^{-1}$
Enthalpy for the reaction $CH_2=CH_2 + H-H \to CH_3-CH_3$ will be .............. $\text{kJ mol}^{-1}$
| $H-H$ bond energy | $431.37 \text{ kJ mol}^{-1}$ |
| $C=C$ bond energy | $606.10 \text{ kJ mol}^{-1}$ |
| $C-C$ bond energy | $336.49 \text{ kJ mol}^{-1}$ |
| $C-H$ bond energy | $410.50 \text{ kJ mol}^{-1}$ |
Enthalpy for the reaction $CH_2=CH_2 + H-H \to CH_3-CH_3$ will be .............. $\text{kJ mol}^{-1}$
MediumAIPMT 2009
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