Final answer:
The change in enthalpy (ΔH) for the freezing of water at -8.00 °C is calculated by multiplying the mass of water by the heat of fusion, which is -332 J/g. Without the mass of water, we can only provide the formula ΔH = m × (-332 J/g), indicating a negative value as it is an exothermic process.
Step-by-step explanation:
To find the change in enthalpy (ΔH) for the freezing of water at -8.00 °C, we must consider the exothermic process of the phase change and the cooling of water from -8.00 °C to its freezing point. The given heat of fusion is -332 J/g, which is the amount of heat released when 1 gram of water freezes.
Since the water is already below 0 °C, we only need to calculate the heat released due to the phase change, not any additional cooling. The change in enthalpy for the freezing process is thus the heat of fusion, ΔH_fus, multiplied by the mass (m) of water we are considering. If the mass of the ice were given, we would proceed with the calculation ΔH = m × ΔH_fus.
However, without knowing the mass of the ice, we cannot determine a specific value for the enthalpy change. Therefore, the answer for ΔH would be the product of the mass and the heat of fusion, with the general answer being ΔH = m × (-332 J/g), noting that this enthalpy change will be negative because freezing is an exothermic process.