Final answer:
The total energy required to heat 100g of ice at -30°C to steam at 300°C is the sum of the energy needed for each step of heating the ice, melting it, heating the water, vaporizing it, and then further heating the steam to the desired temperature.
Step-by-step explanation:
To calculate the energy required to heat 100g of ice at -30°C to steam at 300°C, we need to consider several steps involving temperature changes and phase transitions.
- Heating the ice from -30°C to 0°C.
- Melting the ice at 0°C to water.
- Heating the water from 0°C to 100°C.
- Converting water at 100°C to steam (vaporization).
- Heating the steam from 100°C to 300°C.
Each of these steps requires us to use specific heat capacities or latent heats.
To get the total energy, we sum the energy for each step:
- Q1 = mass * specific heat of ice * ΔT1 (for step 1)
- Q2 = mass * latent heat of fusion (for step 2)
- Q3 = mass * specific heat of water * ΔT2 (for step 3)
- Q4 = mass * latent heat of vaporization (for step 4)
- Q5 = mass * specific heat of steam * ΔT3 (for step 5)
Sum of Q1 through Q5 gives the total energy required.
This process involves the concepts of thermodynamics and calorimetry in Chemistry.