①The amount of heat absorbed (or released) by a process with a temperature change of Δt. Q denotes the amount of heat (J),

Q=c-m-Δt.

Q absorbed=c-m-(t-t0)

Q released=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) (created in honor of the scientist Joule). The unit of heat has historically been defined as the calorie (abbreviated cal, or cal), which is used only as a secondary unit of energy, with 1 cal = 4.184 joules.

Note: 1 kcal = 1,000 calories = 1,000 calories = 4,184 joules = 4.184 kilojoules

The equilibrium relationship maintained between the amount of heat absorbed by an area and the amount of heat released and stored in a given time period.

△ T = (t1-t0)

② solid fuel completely combustion of heat released formula: Q put = mq gas fuel completely combustion of heat released formula: Q = Vq Q represents heat (J), q represents the calorific value ( J / kg ), m represents the mass of solid fuel (kg), V represents the volume of 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)

International Units in the SI System:

Q--. --- the amount of heat given off by the complete combustion of a certain fuel --- joules J

m --- indicates the mass of a certain fuel --- kilogram kg

q --- indicates the calorific value of a certain fuel --- Joules per - joules per kilogram J/kg

The formula for calculating heat energy

(Specific heat capacity is C, mass is m, and Δt is the temperature difference)