Final answer:
The question is about calculating the energy needed to heat 57.0 g of ice at -20°C to water vapor at 131.0°C. Specific heat capacities, heat of fusion, and heat of vaporization are used for each phase change and heating step.
Step-by-step explanation:
The question requires the calculation of the total energy required to convert 57.0 g of ice (H₂O(s)) at -20°C to water vapor (H₂O(g)) at 131.0°C at 1 atm pressure.
The problem can be broken down into several steps: heating the ice to 0°C, melting the ice to water, heating the water to 100°C, vaporizing the water, and finally heating the water vapor to 131.0°C.
Using specific heat capacities and the heat of fusion and vaporization, we can calculate the total heat required.
Without specific heat values for the solid and gaseous states, and the heat of fusion, precise numerical answers cannot be provided.
However, to correctly answer this question, the necessary constants for each phase and transition of water should be used alongside the mass of the water to compute the energy for each state change and heating phase.