What is heat capacity? How is it different from specific heat?

Heat capacity refers to the property of a material to absorb (or emit heat) heat when it is heated (or cooled). The magnitude of the heat capacity is expressed in terms of specific heat capacity (referred to as specific heat).

It can be calculated as follows:

q=cm(t2—t1), so c=q m(t2—t1).

Where: q — heat absorbed or emitted by the material (j); c—specific heat of the material (j (; m — mass of material (g); t2—t1)—the temperature difference (k) before and after the material is heated or cooled.

Specific heat capacity c Significance: The amount of heat absorbed or released by a material with a mass of 1 gram when the temperature rises (or decreases) by 1 k.

The difference between the two: the heat capacity is: the heat capacity q mc, and the magnitude of the heat capacity is equal to the product of the mass of the object and the specific heat.

Thermal specific volume: The amount of heat absorbed (or released) by a unit quantity (mass or volume) of a substance as the temperature increases (or decreases)1, and the monomer is j (kg·).

Mass heat capacity is specific heat.

Heat capacity: The amount of heat absorbed (or released) from the outside world by an object every time the unit temperature rises (decreases) in a certain process. Unit j k.

Specific heat capacity: refers to the heat absorbed by every 1k increase in temperature or the heat emitted by 1k decrease per unit mass when the temperature rises or decreases, unit j.

Therefore, the specific heat capacity is calculated to be more than the upper heat capacity except for one weight.

Heat capacity: heat capacity q mc, the magnitude of the heat capacity is equal to the product of the mass of the object and the specific heat.

Specific heat volume: The amount of heat absorbed (or released) by a unit quantity (mass or volume) of a substance as its temperature rises (or decreases)1 is called the specific heat capacity of the substance. The monomer is j (kg·).

From this point of view, there is a difference between heat capacity and specific heat.

Specific heatThe capacity ratio refers to the constant pressure ratio of the heat cp withVolumetric settingThe ratio of specific heat to CV, usually denoted by symbols, i.e. =cp cv, is an important parameter to describe the thermodynamic properties of gases. According to the theory of molecular motion, the theoretical value is (n+2) n, where n is the degree of freedom of microscopic motion of gas molecules.

number. When an atom gas molecule has only three translational degrees of freedom of motion, i.e., n=3, hence =5 3.

Adiabatic index. Ideal gas.

The index of the reversible adiabatic process is called the adiabatic index, which is denoted by k, so the ideal gas specific heat ratio is equal to the adiabatic index of the Bi Nian hood.

If the fluid working fluid does not exchange heat with the outside world in a certain process of state change, the process is called adiabatic process. When measuring the gas flow rate with a throttle orifice plate, the state change that occurs when the fluid flows through the orifice plate can be approximated as an adiabatic process. In order to find the coefficient of gas expansion in the measurement.

It is necessary to know the adiabatic index that characterizes the adiabatic process of the gas being measured. If the gas can be considered as an ideal gas, then its adiabatic index k is the ratio of the specific heat capacity of the constant pressure to the specific heat capacity of the constant volume, that is, k=cp cv.

Specific heat capacity refers to the amount of heat required to increase the temperature of 1kg of homogeneous substances by 1k when there is no phase change and chemical change.

The ratio of the heat absorbed by a substance of a certain mass to the product of the mass of the substance and the temperature of the substance when the temperature rises is called the specific heat capacity (specific heat) of the substance, which is denoted by the symbol c. The units in the International System of Units are joules per kilogram of Kelvin j (kg·k) or joules per kilogram per kilogram of Celsius j (kg·) j refers to joules and k refers to the thermodynamic temperature scale, i.e., the energy required to raise (or fall) the temperature of 1 kilogram of a substance by 1 Kelvin. q is the heat absorbed (or released); m is the mass of the object, and δt is the amount of change in temperature after endothermic (or exothermic).

Because specific heat is a property of matter, it does not change with the change of external conditions, but is only related to the type of matter and the state of matter.

Different substances can be identified (roughly) by differences in specific heat.

For example, the specific heat capacities of water and oil are about 4200 j (kg·k) and 2000 j (kg·k), respectively, that is, the heat energy of heating water of the same mass is about twice as high as that of oil. If the same mass of water and oil are heated separately with the same heat energy, the temperature rise of the oil will be greater than that of water.