①After a certain process, the temperature changes by △t, and it absorbs (or releases) heat. Q represents the heat(J)
Q=c·m·Δt．
Qsuck=c·m·（t－t0）
Qput=c·m·（t0－t）
（t0is the initial temperature; t is the final temperature）
Where C is the specific heat (capacity) associated with this process．
The unit of heat is the same as the unit of work and energy. In the International System of Units, the unit of heat is the joule (abbreviated as J) (named in honor of the scientist Joule). Historically, the unit of heat was defined as the calorie (abbreviated as cal), which was only used as an auxiliary unit of energy, 1 calorie = 4.184 joules.
Note: 1 kcal = 1000 calories = 1000 calories = 4184 joules = 4.184 kJ
The equilibrium relationship between the heat absorbed by a certain area in a certain period of time and the heat released and stored.
△T=（t1-t0）
②The calculation formula for the heat released by the complete combustion of solid fuel is: Q release = mq The calculation formula for the heat released by the complete combustion of gas fuel is: Q = Vq Q represents heat (J), q represents calorific value (J/kg), m represents the mass of solid fuel (kg), and V represents the volume of gas fuel (m^3).
q = Q release/m (solid); q = Q release/v (gas)
W=Q release=qm=Q release/m W=Q release=qV=Q release/v (W: total power)
(Heating value is related to pressure)
SI international units：
Q———The amount of heat released when a fuel is completely burned - JoulesJ
m———Indicates the mass of a fuel—kilograms kg
q———Indicates the calorific value of a fuel—joules per kilogramJ/kg
Heat energy calculation formula
Q=△t*m*C
(The specific heat is C, the mass is m, and Δt is the temperature difference)
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