Online Calorie Converter Introduction
①The heat absorbed (or released) by a substance undergoing a temperature change of Δt during a process. Q represents 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 capacity associated with this process.
The unit of heat is identical to that of work and energy. In the International System of Units (SI), heat is measured in joules (abbreviated as J) in honor of scientist James Joule. Historically, the calorie (abbreviated as cal) was defined as a unit of heat, though it now serves only as a supplementary unit for energy, with 1 cal = 4.184 J.
Note: 1 kcal = 1000 cal = 1000 calories = 4184 joules = 4.184 kJ
The equilibrium relationship maintained within a given area during a specific time period between the heat absorbed and the heat released or stored.
△T=（t1-t0）
② Formula for heat released during complete combustion of solid fuel: Q_(released) = mq
Formula for heat released during complete combustion of gaseous fuel: Q = Vq
Q represents heat (J), q represents calorific value (J/kg), m represents mass of solid fuel (kg), V represents 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)
(Calorific value is related to pressure)
SI International Units:
Q———Heat released upon complete combustion of a fuel———Joule J
m———Mass of a fuel———Kilogram kg
q———Heat value of a fuel———Joules per kilogram J/kg
Thermal Energy Calculation Formula
Q=△t*m*C
(Specific heat capacity is C, mass is m, temperature difference is Δt)
