Specific heat is define due to dependance of heat capacity on mass.

"Heat capacity per unit mass of a body is known as specific heat of a body".

$s=\frac{\text { Heat capacity }}{\text { Mass of body }}$

$s=\frac{\Delta \mathrm{Q}}{m \Delta \mathrm{T}}$

$\therefore \Delta \mathrm{Q}=m s \Delta \mathrm{T}$

The unit of specific heat is $\mathrm{J} \mathrm{Kg}^{-1} \mathrm{~K}^{-1}$

The magnitude of specific heat depends on the nature of material of body that is on which temperature difference body is stag and in which situation heat is given to the body.

Heat capacity per mole of the substance is known as molar specific heat capacity of a substance,

$\therefore \mathrm{C}=\frac{\mathrm{S}}{\mu}=\frac{1}{\mu} \frac{\Delta \mathrm{Q}}{\mu \Delta \mathrm{T}}$

Here, molar specific capacity is also independent to the amount of substance (mole).

Unit of molar specific capacity is $\mathrm{J} \mathrm{mol}^{-1} \mathrm{~K}^{-1}$.

Here, specific and molar heat capacities of some solids at room temperature and atmospheric pressure is given.

Specific and molar heat capacities of some solids at room temperature and atmospheric pressure:

Substance	Specific Heat $^{-\mathrm{v}}$ ( $\mathrm{J} \mathrm{kg}^{-1} \mathrm{~K}^{-1}$ )	Molar specificHeat $\left(\mathrm{Jmol}^{-1} \mathrm{~K}^{-1}\right)$
Aluminium	$900.0$	$24.4$
Carbon	$506.5$	$6.1$
Copper	$386.4$	$24.5$
Lead	$127.7$	$26.5$
Silver	$236.1$	$25.5$
Tungsten	$134.4$	$24.9$

As table shows, the experimentally measured values which agrees with predicted value $3 \mathrm{R}$ at ordinary temperatures. (Carbon is an exception). The agreement is known to break down at low temperature.