Compute heat change using q = m · c · ΔT (sensible heat).
Heat Energy (q)
4184.00 J
4.1840 kJ · 1.0000 kcal · 3.966 BTU
Formula: q = m · c · ΔT
This tool calculates sensible heat change using the classical thermodynamic relation q = m · c · ΔT. It assumes uniform temperature change across the mass and uses the specific heat capacity provided. Specific heat varies with material and temperature; the default value shown is for liquid water at typical temperatures. For combustion energy (higher-order energetic content), use tabulated heats of combustion per mass of the fuel.
Use results to estimate energy transfer for heating or cooling processes, calorimetry checks, and simple engineering approximations. Remember that real systems may have heat losses, non-uniform temperature distributions, and phase changes which are not included here.
q = m · c · ΔT where m is mass, c is specific heat, and ΔT is temperature change.
Outputs include J, kJ, kcal, and BTU; mass shown in g, kg, and lb.
kcal is commonly used in chemistry and food energy contexts for human-readable energy values.
Heat is zero if mass or ΔT is zero; negative or zero mass is invalid for this tool.
Enter mass in grams; use the kg output for confirmation (mass in kg = g ÷ 1000).
Conversions use standard factors (1 kJ = 1000 J, 1 kcal = 4184 J, 1 BTU ≈ 1055.06 J).
This computes sensible heat change (q). Heat of combustion is typically reported per mass on a different basis — consult material tables for true heat of combustion.
Handle energetic materials with care; use appropriate safety and regulatory guidance when interpreting energy numbers.
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