The change in entropy when 55 g of water (the latent heat of vaporization of water is 22.6 * 10⁵ J/kg) at 100°C is turned into steam at 100°C is

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The change in entropy ($\Delta S$) during the phase change from liquid to gas can be calculated using the formula $\Delta S = \frac{Q}{T}$, where $Q$ is the heat absorbed or released during the phase change, and $T$ is the absolute temperature in Kelvin. For water turning into steam, $Q = m \cdot L$, where $m$ is the mass of the water and $L$ is the latent heat of vaporization. Given that $m = 55$ g (or 0.055 kg) and $L = 2260 \times 10^3$ J/kg, $Q = 0.055 \times 2260 \times 10^3 = 124300$ J. Since the process occurs at $100^\circ C$ or $373 K$, $\Delta S = \frac{124300}{373} \approx 333$ J/K.

The Change in Entropy When 55 G of Water (The