To determine the amount of steam required to melt 1 kg of ice at 0°C, we need to consider the energy transfer involved in the phase change from ice to water.
To calculate the energy required to melt the ice, we can use the specific latent heat of fusion for water. The specific latent heat of fusion (Lf) is the amount of energy required to change 1 kg of a substance from a solid to a liquid at its melting point.
For water, the specific latent heat of fusion is approximately 334,000 joules per kilogram (J/kg).
First, we need to calculate the energy required to melt 1 kg of ice:
Energy required = mass of ice × specific latent heat of fusion
Energy required = 1 kg × 334,000 J/kg
Energy required = 334,000 joules
Now, we need to determine the amount of steam required to provide this energy. To do that, we'll use the specific enthalpy of steam.
The specific enthalpy of steam at 150°C can be determined based on the properties of steam. However, the specific enthalpy values can vary depending on the steam pressure and other factors. Assuming the steam is at atmospheric pressure, we can use an approximate value of 2,257 kilojoules per kilogram (kJ/kg) for the specific enthalpy of steam at 150°C.
Now, we can calculate the amount of steam required:
Mass of steam = Energy required ÷ specific enthalpy of steam
Mass of steam = 334,000 J ÷ 2,257,000 J/kg
Mass of steam ≈ 0.148 kg
Therefore, approximately 0.148 kg of steam at 150°C is needed to melt 1 kg of ice at 0°C.