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Calorimetry is the measurement of heat transfer. The key formula is $Q = mc\Delta T$ for sensible heat (no change of state) and $Q = mL$ for latent heat (change of state). Specific heat capacity $c$ is the heat required…
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Describe an experiment to determine the specific heat capacity of a solid using the method of mixtures.
Heat a known mass of solid to a known temperature, mix with water in a calorimeter, measure final temperature, and apply heat lost = heat gained.
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A calorimeter of mass 50 g (specific heat 400 J kg⁻¹ K⁻¹) contains 150 g of water at 30°C. Steam at 100°C is passed into it until the temperature becomes 40°C. Find the mass of steam condensed. (Latent heat of vaporisation = 2260000 J kg⁻¹)
Heat gained = (0.05×400+0.15×4200)×(40−30) = 6500 J; heat lost by steam = m×2260000 + m×4200×(100−40) = m×(2260000+252000) = m×2512000; m = 6500/2512000 ≈ 0.00259 kg = 2.59 g.
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A 500 g block of copper at 80°C is placed in a calorimeter of water equivalent 25 g containing 300 g of water at 20°C. Find the final temperature. (Specific heat of copper = 400 J kg⁻¹ K⁻¹)
Heat lost = 0.5×400×(80−T); heat gained = (0.3+0.025)×4200×(T−20); equate: 200(80−T)=1365(T−20) → T ≈ 27.6°C.
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State and explain the three modes of heat transfer. Give one example of each.
Conduction (solid), convection (fluid), radiation (no medium); examples: metal rod, sea breeze, sun's heat.
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A piece of metal of mass 200 g is heated to 100°C and then dropped into 400 g of water at 20°C in a calorimeter of water equivalent 20 g. The final temperature is 25°C. Calculate the specific heat capacity of the metal.
Using heat lost = heat gained: 0.2 × c × (100−25) = (0.4+0.02) × 4200 × (25−20) → c = 882 J kg⁻¹ K⁻¹.
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How much heat is required to convert 100 g of ice at −10°C to steam at 100°C? (Specific heat of ice = 2100 J kg⁻¹ K⁻¹, latent heat of fusion = 336000 J kg⁻¹, specific heat of water = 4200 J kg⁻¹ K⁻¹, latent heat of vaporisation = 2260000 J kg⁻¹)
Total heat = (0.1×2100×10) + (0.1×336000) + (0.1×4200×100) + (0.1×2260000) = 301000 J.
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Explain the concept of latent heat with the help of a heating curve for water.
Heating curve shows temperature vs time; flat regions indicate phase changes where heat is latent.
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Differentiate between specific heat capacity and heat capacity.
Specific heat capacity is per unit mass, heat capacity is for the whole body; units J kg⁻¹ K⁻¹ vs J K⁻¹.
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Explain why the climate near the sea is moderate compared to inland areas.
Water has high specific heat capacity; it heats and cools slowly, moderating coastal temperatures.
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Define specific heat capacity of a substance.
It is the amount of heat required to raise the temperature of 1 kg of the substance by 1°C (or 1 K).
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Define latent heat of fusion.
It is the heat required to convert 1 kg of a solid into liquid at its melting point without any change in temperature.
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State the principle of mixtures.
Heat lost by hotter bodies equals heat gained by colder bodies, provided no heat is lost to the surroundings.
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Why does temperature remain constant during a phase change?
Because the heat supplied is used to overcome intermolecular forces (latent heat) and not to increase kinetic energy.
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What is meant by 'water equivalent' of a calorimeter?
It is the mass of water that would require the same heat as the calorimeter to raise its temperature by 1°C.
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Why is water used as a coolant in car radiators?
Because water has a high specific heat capacity, it can absorb a large amount of heat without a large rise in temperature.
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State the SI unit of specific heat capacity.
J kg⁻¹ K⁻¹ (or J kg⁻¹ °C⁻¹).
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What is the specific heat capacity of water?
4200 J kg⁻¹ K⁻¹ (or 4.2 J g⁻¹ °C⁻¹).
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State the latent heat of vaporisation of water.
2260 kJ kg⁻¹ (or 2.26 × 10⁶ J kg⁻¹).
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Write the formula for heat required to change the temperature of a body without change of state.
$Q = mc\Delta T$
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