Final answer:
The final temperature of the ice after absorbing 70 kJ of energy will exceed 0°C as the energy released is sufficient to both warm the ice from -10°C to 0°C and melt it. However, without additional information such as the specific heat capacity of water, the exact final temperature cannot be determined.
Step-by-step explanation:
To determine the final temperature of 100.0 g of ice starting at -10°C and absorbing 70 kJ of energy, we must consider the specific heat capacity of ice and the heat of fusion. Ice has a specific heat capacity of approximately 2.09 J/g°C, which means it requires 2.09 J to raise the temperature of 1 gram of ice by 1°C. The heat of fusion of ice is about 334 J/g, the amount of energy needed to melt 1 gram of ice at its melting point without changing its temperature.
We will approach this problem in two stages: First, we will calculate the energy required to warm the ice from -10°C to 0°C. Then, we'll use any remaining energy to melt the ice.
Energy to warm the ice:
Since 2.09 kJ is needed to warm the ice to 0°C, we'll subtract this from the 70 kJ provided.
70 kJ - 2.09 kJ = 67.91 kJ remaining
Energy to melt the ice (if any is left):
Since we have 67.91 kJ remaining and only need 33.4 kJ to melt the ice, all the ice will melt. After all the ice is melted into water, any remaining energy will then start to warm the water. As there is still some energy left, the final temperature will be above 0°C, but a specific final temperature cannot be determined with the information provided as we need the specific heat capacity of water to calculate this.