Introduction to the online heat converter

1, After a process the temperature change is △t, and the heat it absorbs (or releases). Q denotes the heat (J)

Q=c·m·Δt．

Q (absorbed) = c·m·(t - t0)

Q放=c·m·（t0－t）

(t0 is the initial temperature; t is the final temperature)

where C is the specific heat related to this process.

The unit of heat is the same as that of work and energy. In the SI system the unit of heat is the joule (abbreviated J, named after the scientist Joule). Historically the calorie (abbreviated cal) was defined as an auxiliary unit of energy, where 1 cal = 4.184 J.

Note: 1 kilocalorie=1000 cal=1000 calories=4184 joules=4.184 kilojoules

The balance maintained between the heat a region absorbs in a period and the heat it releases and stores.

△T=（t1-t0）

2. Formula for the heat released by the complete combustion of solid fuel: Q=mq. Formula for the heat released by the complete combustion of gaseous fuel: Q=Vq. Q is the heat (J), q the calorific value (J/kg), m the mass of the solid fuel (kg) and V the volume of the gaseous fuel (m^3).

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)

(heat value depends on pressure)

SI units:

Q——— the heat released after complete combustion of a kind of fuel ——— joules J

m - the mass of a kind of fuel - kilograms kg

q——— the calorific value of a kind of fuel ——— joules per kilogram J/kg

Heat formula

Q=△t*m*C

(specific heat is C, mass is m, Δt is the temperature difference)