①The change in temperature by a certain process is △t, the amount of heat it absorbs (or emits). q denotes the amount of heat (J)
Q=c·m·Δt．
Q absorb = c-m-(t-t0)
Q put = c - m - (t0 - t)
(t0 is the initial temperature; t is the final temperature)
Where C is the specific heat (volume) associated with the process.
The units of heat are the same as those of work and energy. The unit of heat in the International System of Units is the joule (abbreviated Joule, abbreviated J) (established in honour of the scientist Joule). Historically, the unit of heat was defined as the calorie (abbreviated calorie, abbreviated cal), which is used only as a secondary 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 and the heat released and stored in an area at a given time is maintained.
△T=（t1-t0）
② The formula for calculating the amount of heat released by the complete combustion of a solid fuel: Q put = mq The formula for calculating the amount of heat released by the complete combustion of a gaseous fuel: Q = Vq Q denotes the amount of heat (J), q denotes the calorific value ( J/kg ), m denotes the mass of the solid fuel (kg), and V denotes the volume of the gaseous fuel (m^3).
q=Q discharge/m (solid); q=Q discharge/v (gas)
W=Q discharge = qm = Q discharge/m W=Q discharge = qV = Q discharge/v (W: total work)
(Calorific value is related to pressure)
SI system of international units:
Q - the amount of heat given off by the complete combustion of a certain fuel - Joule J
m --- indicates the mass of a fuel --- kilogram kg
q - indicates the calorific value of a fuel - Joule per kg J/kg
Calculation formula for heat energy
Q=△t*m*C
(Specific heat capacity is C, mass is m, Δt is temperature difference)