Two kilograms of water at 1.00 atm at the boiling point of 100$\degree$C is heated until all the water vaporizes. What is its change in entropy? (For water, L_v = 2.26 * 10⁶ J/kg)

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Quizplus · Accepted Answer

The change in entropy is given by:$$\Delta S = \frac{L_v}{T}$$where:* $L_v$ is the latent heat of vaporization* $T$ is the temperaturePlugging in the given values, we get:$$\Delta S = \frac{2.26 	imes 10^6 	ext{ J/kg}}{373 	ext{ K}} = 6060 	ext{ J/K}$$

Two Kilograms of Water at 1 °\degree° C Is Heated Until All the Water Vaporizes

Two Kilograms of Water at 1 $\degree$ C Is Heated Until All the Water Vaporizes