Standard Enthalpy Of Formation, Combustion And Bond Dissociation MCQ

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Enthalpy Of Combustion, Enthalpy Of Dissociation, Atomisation And Phase Change is considered one of the most asked concept.
28 Questions around this concept.

Concepts Covered - 2

Enthalpy Of Combustion

Heat of Combustion

1. It is, changes in enthalpy when one mole of a substance is completely oxidized or combusted or burnt.

2. $\mathrm{\Delta H}$ is - ve here as heat in always evolved here that is, exothermic process.

3. Heat of combustion is useful in calculating the calorific value of food and fuels.

4. It is also useful in confirming structure of organic molecules having C,H,O,N etc.

5. Enthalpy change by combustion of 1 gm solid or 1 gm liquid or 1 cc gas is called calorific value.

$\mathrm{calorific\ value}=\frac{\text { Heat of combustion }}{\text { Molecular wt. }}$

$\Delta \text {H (heat of reaction) }=-\Sigma \Delta \mathrm{H}_{\mathrm{P}}^{\mathrm{o}}-\Sigma \mathrm{H}_{\mathrm{R}}^{\mathrm{o}}$

Enthalpy Of Dissociation, Atomisation And Phase Change

Enthalpy of Dissociation or Ionization

It is defined as, "The quantity of heat absorbed when one mole of a substance is completely dissociated into its ions". Example,

Heat of Atomization

It is the enthalpy change (heat required) when bonds of one mole of a substance are broken down completely to obtain atoms in the gaseous phase (isolated) or it is the enthalpy change when one mole of atoms in the gas phase is formed from the corresponding element in its standard state. In case of diatomic molecules, it is also called bond dissociation enthalpy.

Phase Transition and Transition Energy

The change of matter from one state (solid, liquid or gas) to another state is called Phase Transition.
Such changes occur at definite temperatures such as meltmg point (solid to liquid), bolling point (liquid to vapours) etc., and are accompanied by absorption or evolution of heat. The enthalpy change during such phase transitions is called heat of transltion or transition energy.