Specific Heat Capacity Calculator (Q = mcΔT)

Specific Heat Capacity Guide

Q = mcΔT

Q = m × c × ΔT. Where Q = heat energy transferred (joules, J), m = mass (kg), c = specific heat capacity (J/kg·K), ΔT = temperature change (°C or K — the size of a degree is the same). Note: if mass is in grams, convert to kg (divide by 1000). Specific heat capacity: the energy needed to raise 1 kg of a substance by 1°C. Water (4,181 J/kg·K) has an unusually HIGH specific heat — making it excellent for heating systems and for life (bodies are mostly water). Metals have low c values — they heat u

Calorimetry

Calorimetry measures heat transfers: a known mass of water in a known mass of calorimeter absorbs heat from a reaction or burning material. Calculate Q_water = m_water × c_water × ΔT. For an insulated calorimeter, Q_reaction = −Q_water. Then molar enthalpy: ΔH = Q / moles of substance. Sources of error: heat loss to surroundings (use insulation, polystyrene cups). Incomplete combustion (in spirit burner experiments). Evaporation of fuel. Systematic error: specific heat of the calorimeter itself

Water's Unusual Properties

Water's high specific heat capacity (4,181 J/kg·K) has profound consequences: climate moderation: coastal areas have smaller temperature ranges than inland areas — the ocean absorbs and releases heat slowly. Sweating: evaporating 1g of water removes 2,256 J from the body. Human body temperature regulation. Central heating: water efficiently transports heat from boiler to radiators (1L carries 4,181 J per degree). Hydroelectric storage: pumped storage uses water as a thermal and gravitational ene

Phase Changes

Q = mcΔT only applies during temperature change — NOT during phase changes (melting/boiling). During a phase change, temperature stays constant while energy is absorbed or released. Latent heat formula: Q = mL. Where L = specific latent heat. Latent heat of fusion (ice→water): L_f = 334,000 J/kg. Latent heat of vaporisation (water→steam): L_v = 2,260,000 J/kg. Example: melting 1kg of ice at 0°C then heating to 100°C then boiling: Q_melt = 1 × 334,000 = 334 kJ. Q_heat = 1 × 4,181 × 100 = 418.1 kJ