Final answer:
The heat of fusion of ice is approximately 4.184 J/g.
Step-by-step explanation:
To calculate the heat of fusion of ice, we can use the formula:
Q = m * ΔH_fusion
where Q is the heat absorbed or released during the phase change, m is the mass of the ice, and ΔH_fusion is the heat of fusion of ice.
In this case, we know the mass of the ice is 0.15 kg and the resulting temperature is 6.7 °C, which is above the melting point of ice. So, the heat released by the ice to cool down and melt into water can be calculated using the formula:
Q = m * c * ΔT
where c is the specific heat capacity of water and ΔT is the change in temperature.
Since the resulting temperature is above the melting point of ice, we can assume that all the ice has melted. Therefore, the heat released by the ice is equal to the heat absorbed by the resulting mixture. By equating the two expressions for Q, we can solve for ΔH_fusion.
Q = m * ΔH_fusion
m * c * ΔT = m * ΔH_fusion
ΔH_fusion = (m * c * ΔT) / m
Substituting the given values:
ΔH_fusion = (0.15 kg * 4.184 J/(g·°C) * (6.7 °C - 0 °C)) / 0.15 kg
Simplifying the expression, we find:
ΔH_fusion = 4.184 J/g
Therefore, the heat of fusion of ice is approximately 4.184 J/g.