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).