Final answer:
To calculate Gibbs free energy (ΔG), use the equation ΔG = ΔH - TΔS. Apply the correct values for enthalpy, entropy, and temperature, remembering that at equilibrium between two phases, ΔG equals zero. For transitions between steam and ice, steam loses entropy and gains order, while ice gains entropy and loses order.
Step-by-step explanation:
To calculate the Gibbs free energy for ice, water, and steam, you should use the following equation:
ΔG = ΔH - TΔS
This equation takes into account the enthalpy change (ΔH) and the entropy change (ΔS) for the system, with ΔG representing the change in free energy. It's essential to use the correct values for specific heat, enthalpy of fusion (ΔHfus), enthalpy of vaporization (ΔHvap), and absolute temperature (in Kelvin) to accurately calculate ΔG for each state transition (ice to water, water to steam).
For instance, at the equilibrium between ice and water at 0°C, the Gibbs free energy change (ΔG) is equal to zero. If we know the heat of fusion of water (6.01 kJ/mol), we can solve for the entropy change during melting (ΔSfus) using the same equation.
When steam and ice are placed in contact, as described in the hypothetical scenario, the steam will lose entropy and order, while the ice will gain entropy and lose order. Therefore, the correct answer for that specific process would be b. gained, lost, lost, gained.