$$c = \dfrac{Q}{m \Delta T}$$
where $c$ is the specific heat capacity of the substance (in J kg-1 $\degree$C-1),
$Q$ is the heat transfer or energy absorbed (in J),
$m$ is the mass of the substance (in kg), and
$\Delta T$ is the change in temperature (in $\degree$C or K)
It is an intrinsic property of the material and is independent of the amount of substance. Different substances have different specific heat capacities, which reflect how much energy is required to change their temperatures. The following is a table of some of the commonly known specific heat capacities.
| Substance | Specific Heat Capacity (J kg-1°C-1) |
|---|---|
| Water | 4186 |
| Ice | 2100 |
| Aluminum | 897 |
| Iron | 450 |
| Copper | 385 |
| Lead | 128 |
| Air | 1005 |
| Ethanol | 2440 |
To calculate the amount of thermal transfer $Q$ needed to raise a substance of specific heat capacity $c$ and mass $m$ by a temperature change of $\Delta T$, we can use this formula: $$Q = mc\Delta T$$
Heat capacity, $C$, is the amount of energy needed to raise the temperature of an object by 1 $\degree$C or 1 K. Unlike specific heat capacity, heat capacity depends on the mass of the object. For an object of mass $m$ made of a substance with specific heat capacity $c$, its heat capacity is given by $$C = mc$$