Final answer:
After melting 150g of ice at 0°C with 75.0 kilojoules of energy, all ice will melt and the remaining energy will raise the temperature of the resulting water to approximately 39.7°C.
Step-by-step explanation:
To determine the final temperature of water after adding 75.0 kilojoules of energy to 150g of ice at 0.0°C, we need to calculate how much of that energy is used to melt the ice and how much is used to raise the temperature of the resulting water. The heat of fusion for ice is 334 J/g, which is the amount of energy needed to melt 1g of ice into 1g of water at 0°C. First, we find out how much ice can be melted with 75.0 kJ:
- 75.0 kJ = 75,000 J
- 75,000 J / 334 J/g = approximately 224.6g of ice
Since only 150g of ice is available, all of it will melt, requiring:
- 150g * 334 J/g = 50,100 J
After melting, we have 50,100 J remaining from the initial energy to raise the temperature of the water:
- 75,000 J - 50,100 J = 24,900 J left to heat the water
Using the specific heat capacity of water, which is 4.18 J/g°C, we can then calculate the increase in temperature:
- 24,900 J / (150g * 4.18 J/g°C) = approximately 39.7°C
Therefore, the water will be heated beyond its melting point up to a final temperature of 39.7°C.