1 g of water, of volume 1 cm³ at 100°C, is converted into steam at same temperature under normal atmospheric pressure (1 × 10⁵ Pa). The volume of steam formed equals 1671 cm³. If the specific latent heat of vaporisation of water is 2256 J/g, the change in internal energy is,

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2089 J. The work done during expansion is W = PΔV = (1 × 10⁵ Pa)(1671 - 1) × 10⁻⁶ m³ = 0.167 J. The heat absorbed is Q = mL = (1 g)(2256 J/g) = 2256 J. Using the first law of thermodynamics, ΔU = Q - W = 2256 J - 167 J = 2089 J.

1 g of water, of volume 1 cm³ at 100°C, is converted into steam at same temperature under normal atmospheric pressure (1 × 10⁵ Pa). The volume of steam formed equals 1671 cm³. If the specific latent heat of vaporisation of water is 2256 J/g, the change in internal energy is,

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