Specific heat capacity

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The **energy needed to raise the temperature of 1 kg of a substance by 1 degree** (1 K). Unit: J kg⁻¹ K⁻¹.

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**J kg⁻¹ K⁻¹** (joules per kilogram per kelvin: the energy to raise 1 kg by 1 K, i.e. 1 °C).

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$Q = mc\Delta T$ — mass × specific heat capacity × temperature change. **Given** in the data booklet.

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The temperature **change** = final temperature − start temperature (Δ means 'change in').

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**No** — a change of 1 K is the same size as a change of 1 degree C, so either works. Never convert ΔT to kelvin.

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$c = \dfrac{Q}{m\,\Delta T}$ — energy ÷ (mass × temperature change).

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$m = \dfrac{Q}{c\,\Delta T}$.

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Is **hard to heat** — it needs lots of energy per degree, so it warms and cools **slowly** (like water).

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It has a **very large** specific heat capacity (about 4200 J kg⁻¹ K⁻¹), so it absorbs a lot of energy with only a small temperature rise.

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During a **change of state** (melting/boiling), where the temperature stays constant — use $Q = mL$ instead.

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Putting the **actual temperature** into ΔT instead of the **change** (final − start).

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**Q = Pt = IVt**, with t in seconds.

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Energy lost by the hot body = energy gained by the cold body: **m₁c₁ΔT₁ = m₂c₂ΔT₂**.

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Energy is lost to the surroundings, so the block gains less than IVt, but all of IVt is used as Q.