How much energy is released or absorbed when $1 g m$ of steam at $100^{\circ} C$ turns to ice at $0^{\circ} C$ ?

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Solution

Energy released = Energy for state change from steam to water at $100^{0} C$ + Energy for temperature change from $100^{0} C$ to $0^{0} C$ + Energy for state change from water to ice state change at $0^{0} C$ .
$Q = m L_{v a p o u r i s a t i o n} + m s Δ T + m L_{f u s i o n}$
$m = 1 g m, Δ T = 100 K, L_{v a p o u r i s a t i o n} = 2257 J / g m, L_{f u s i o n} = 334 J / g m, s = 4.2 J g m^{- 1} K^{- 1}$
$Q = 2257 + 420 + 334 = 3011 J$

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