# Heat Capacity

## The heat capacity of a substance is the amount of heat required to change its temperature by one degree, and has units of energy per degree

**Heat Capacity** - *C* - is a characteristic of an object -* the amount of heat required to change its temperature by one degree.*

- Heat Capacity has the units of energy per degree.

The amount of heat supplied to heat an object can be expressed as:

Q = C dt (1)

where

Q = amount of heat supplied (J, Btu)

C = heat capacity of system or object (J/K, Btu/^{o}F)

dt = temperature change (K, C°,^{o}F)

The SI unit for heat capacity is J/K (joule per kelvin). In the English system, the units are British thermal units per pound per degree Fahrenheit (Btu/^{o}F). In some contexts kJ or cal and kcal are used instead of J.

*Never use tabulated values of heat capacity without checking the unit of actual values!*

**Specific Heat Capacity**

**(**is the amount of heat required to change the temperature of a mass unit of a substance by one degree.

*c*)**Specific heat**is a more common term for the same.

The heat supplied to a mass can be expressed as

*dQ = m c dt (1)*

*where*

*dQ = heat supplied (J, kJ Btu)*

*m = unit mass (g, kg, lb)*

*c = specific heat (J/g K, kJ/kg ^{ o}C, *

*kJ/kg*

^{ }K,*Btu/lb*

^{ o}F)*dt = temperature change (K, C °, ^{o}F)*

*(1)* can be transferred to express Specific Heat as:

**c = dQ / m dt ** (1b)

**Example:** The specific heat of iron is 0.45 J/(g K), which means that it takes 0.45 Joules of heat to raise one gram of iron by one degree Kelvin.

Download and print Heat supplied vs. Specfic heat and change in Temperature chart

**Specific Heat Gases**

There are two definitions of Specific Heat for vapors and gases:

c_{p}= (δh / δT)_{p}- Specific Heat at constant pressure (J/gK)

c_{v}= ( δh / δT)_{v}- Specific Heat at constant volume (J/gK)

For solids and liquids, c_{p} = c_{v}

Use the links to see *tabulated values of specific heat* of gases, common liquids and fluids, food and foodstuff, metals and semimetals, common solids and other common substances.

Gas Constant

The individual individual gas constant, R, can be expressed as

R = c_{p}- c_{v}(2)

Ratio of Specific Heat

The Ratio of Specific Heat is expressed as

k = c_{p}/ c_{v}(3)

Molar Heat Capacity**( C_{p})** is the amount of heat needed to increase the temperature of

*one mol*of a substance by one degree at constant pressure.

It is expressed in joules per moles per degrees Kelvin (or Celsius),

*J/(mol K)*.

**Example:** The molar heat capacity of iron is 25.10 J/(mol K), which means that it takes 25.10 Joules of heat to raise 1 mol of iron by 1 degree Kelvin.

Tabulated values of molar heat capacity, C_{p,} of a lot of organic and inorganic substances can be found in Standard enthalpy of formation, Gibbs free energy of formation, entropy and molar heat capacity of organic substances and Standard state and enthalpy of formation, Gibbs free energy of formation, entropy and heat capacity, together with ΔH°_{f}, ΔG°_{f} and S° for the same substances at 25°C.

**Converting between Specific heat and Molar heat capacity**

The specific heat capacity can be calculated from the molar heat capacity, and vise versa:

*c _{p} = C_{p} / M and *

*C _{p} = c_{p} ^{.} M*

_{}

*where*

*c _{p} = specific heat capacity*

*C _{p} = molar heat capacity*

*M = molar weight of the actual substance (g/mol).*

**Example: **Methanol (with molecular formula CH3OH) has a molar heat capacity, C_{p}, of 81.1 J/(mol K). What is the specific heat capacity, c_{p}?

First, we calculate (or find) the molar weight of methanol: 1*12.01g/mol C + 4*1.008g/mol H + 1*16.00g/mol O = *32.04 g/mol CH _{3}OH*

Then, the specific heat capacity of methanol is: **c _{p}** = 81.8 J/(molK) / 32.04 g/mol =

**2.53 J/(g K)**

**Converting between commonly used Units**

*1 Btu/lb*_{m}^{o}F = 4186.8 J/kg K = 1 kcal/kg^{o}C- Online Specific heat capacity unit converter

Example - Heating Aluminum

*2 kg* of aluminum is heated from *20 ^{o}C to 100 ^{o}C*. Specific heat of aluminum is

*0.91 kJ/kg*and the heat required can be calculated as

^{0}C*dQ = (2 kg) (0.91 kJ/kg ^{0}C) ((100 ^{o}C) - (20 ^{o}C)) *

* = 145.6 (kJ)*

#### Example - Heating Water

*One liter* of water is heated from *0 ^{o}C* to boiling

*100*. Specific heat of water is

^{o}C*4.19 kJ/kg*and the heat required can be calculated as

^{0}C*dQ = (1 litre) (1 kg/litre) (4.19 kJ/kg ^{0}C) ((100 ^{o}C) - (0 ^{o}C)) *

* = 419 (kJ)*

* = 419 (kWs) (1/3600 h/s)*

* = 0.12 kWh*

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