500-g of water at 100 $\circ$ C is changed into steam at 100 $\circ$ C at constant pressure.The change in entropy of the water is

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The change in entropy ($\Delta S$) when water is converted to steam at constant temperature and pressure can be calculated using the formula $\Delta S = \frac{Q}{T}$, where $Q$ is the heat absorbed and $T$ is the absolute temperature in Kelvin. The heat absorbed ($Q$) can be found from the latent heat of vaporization of water, which is approximately 2260 kJ/kg at 100°C. Since we have 500 g (or 0.5 kg) of water, $Q = 0.5 \times 2260 = 1130$ kJ. The temperature $T$ must be in Kelvin, so we convert 100°C to Kelvin by adding 273.15, giving us 373.15 K. Thus, $\Delta S = \frac{1130}{373.15}$ kJ/K, which is approximately 3.03 kJ/K.

500-G of Water at 100 ∘\circ∘ C Is Changed into Steam at 100

500-G of Water at 100^$\circ$C Is Changed into Steam at 100