Calculate the change in entropy that occurs in the system when 55.0 g of water vaporizes from a liquid to a gas at its boiling point (100.0 °C). See Table 11.7 for heats of vaporization.

Verified step by step guidance

1. <Determine the number of moles of water: Use the molar mass of water (18.02 g/mol) to convert the mass of water (55.0 g) into moles.>
2. <Identify the heat of vaporization: Look up the heat of vaporization for water at its boiling point, which is typically given in kJ/mol.>
3. <Calculate the total heat absorbed: Multiply the number of moles of water by the heat of vaporization to find the total heat absorbed during the phase change.>
4. <Convert the heat absorbed to the same units as entropy: Since entropy is often expressed in J/K, convert the total heat absorbed from kJ to J.>
5. <Calculate the change in entropy: Use the formula \( \Delta S = \frac{q_{rev}}{T} \), where \( q_{rev} \) is the heat absorbed (in J) and \( T \) is the temperature in Kelvin (373 K for water at boiling point).>