① The temperature change during a process is represented by △t, and the heat absorbed (or released) is indicated by Q.
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)
Here, C represents the specific heat capacity associated with the process.
The unit of heat is the same as that of work and energy. In the International System of Units (SI), the unit of heat is the joule (abbreviated as J), named after the scientist James Prescott Joule. Historically, the calorie (abbreviated as cal) was defined as a unit of heat, used as an auxiliary unit of energy: 1 cal = 4.184 J.
Note: 1 kilocalorie = 1000 calories = 4184 joules = 4.184 kilojoules
The balance of heat absorbed and released in a certain area over a specific period.
△T = (t1 - t0)
② The calculation formula for the heat released during the complete combustion of solid fuels: Q released = mq, and for gaseous fuels: Q = Vq. Here, Q indicates heat (J), q is the calorific value (J/kg), m is the mass of solid fuel (kg), and V is the volume of gaseous fuel (m³).
q = Q released/m (solid); q = Q released/V (gas)
W = Q released = qm = Q released/m W = Q released = qV = Q released/V (W: total work)
(The calorific value is related to pressure)
SI International Units:
Q — heat released after the complete combustion of a fuel — joules J
m — mass of a specific fuel — kilograms kg
q — calorific value of a specific fuel — joules per kilogram J/kg
Heat Energy Calculation Formula
Q = △t*m*C
(Specific heat capacity is C, mass is m, and Δt is the temperature difference)