Final answer:
The entropy change of 10 g of steam at 100°C when it condenses to water at the same temperature is approximately 60.6 J/K.
Step-by-step explanation:
The entropy change of 10 g of steam at 100°C when it condenses to water at the same temperature can be calculated using the equation:
ΔS = q/T
Where ΔS is the change in entropy, q is the heat transferred, and T is the temperature in Kelvin. To solve this problem, we need to know the heat transferred when the steam condenses to water. This can be calculated using the formula:
q = m * L
Where q is the heat transferred, m is the mass of the substance, and L is the latent heat of vaporization. In this case, the latent heat of vaporization is the energy required to change 1 g of steam to water at 100°C, which is 2260 J/g. Therefore, the heat transferred is 10 g * 2260 J/g = 22600 J. The change in entropy is then calculated as follows:
ΔS = 22600 J / 373.15 K = 60.6 J/K
Therefore, the entropy change of 10 g of steam at 100°C when it condenses to water at the same temperature is approximately 60.6 J/K.