Final answer:
Using the heat of fusion for water (6.01 kJ/mol), 0.400 kJ of energy can melt approximately 1.198 grams of ice, which does not align with the provided options, indicating a possible error in the question or options.
Step-by-step explanation:
To determine how many grams of ice at 0°C can be melted by the addition of 0.400 kJ of heat, we first need to consider the heat of fusion for water, which is 6.01 kJ/mol. This value represents the amount of energy required to melt one mole of ice.
Since the molar mass of water (ℓ₂O) is approximately 18.015 g/mol, we can calculate the number of moles that 0.400 kJ can melt as follows:
Moles of ice melted = Heat added / Heat of fusion = 0.400 kJ / 6.01 kJ/mol
This gives us approximately 0.06656 moles of ice that can be melted. Finally, we convert the moles of ice into grams:
Grams of ice melted = Moles of ice melted × Molar mass of water = 0.06656 moles × 18.015 g/mol
The result is approximately 1.198 g of ice that can be melted, which does not match any of the options provided, suggesting there may have been a mistake or typo in the options or the initial setup of the problem. Typically, in questions like this, we would expect the calculations to yield a result that aligns with one of the provided options.