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Answer :
The energy required to convert 1.70 g of ice originally at -12°C into steam at 105°C is approximately 6162.95 Joules.
To calculate this energy, we need to consider the different energy changes involved in each phase transition. First, we calculate the energy required to heat the ice from -12°C to its melting point at 0°C using the specific heat capacity of ice. Then, we calculate the energy required to melt the ice at 0°C using the heat of fusion for ice. Next, we determine the energy needed to heat the resulting water from 0°C to 100°C using the specific heat capacity of water. Finally, we calculate the energy required to convert the water at 100°C into steam at 105°C using the heat of vaporization for water. Adding up all these energy changes, we find that the total energy required is approximately 6162.95 Joules. This calculation takes into account the various temperature changes and phase transitions that the substance undergoes. It highlights the significant amount of energy needed to convert ice to steam, involving both the heating of the substance and the energy required to change its state.
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