Question

If the heat of fusion for water is 334 J/g, how many kilojoules are lost when 45.0 g of water at 0.0 °C is converted to ice at 0.0 °C?

Answer 1

When 45.0 g of water is converted to ice at 0.0 °C, the total energy lost is 15.030 kilojoules, calculated by using the heat of fusion for water, which is 334 J/g.

Step-by-step explanation:

The amount of energy required to convert water to ice is directly related to the heat of fusion. The heat of fusion for water is given as 334 J/g. To find out how much energy is lost when 45.0 g of water is converted to ice at the same temperature, you multiply this value by the mass of the water:

Energy (E) = mass (m) × heat of fusion (Lf)

E = 45.0 g × 334 J/g

E = 15030 J

To convert this amount into kilojoules, you divide by 1000:

E = 15.030 kJ

So, the total amount of energy lost when 45.0 g of water at 0.0 °C is converted to ice at 0.0 °C is 15.030 kilojoules.