To calculate the amount of heat required to evaporate the water formed from 10g of ice at 0°C, we need to consider the heat needed for the phase change from solid to liquid (melting) and the heat needed for the phase change from liquid to gas (vaporization).
- Heat for melting (ice to water): The heat required for melting can be calculated using the formula: Q = m * Lf where Q is the heat required, m is the mass of the ice, and Lf is the specific latent heat of fusion for ice. The specific latent heat of fusion for ice is approximately 334 J/g.
Q_melting = 10g * 334 J/g = 3340 J
- Heat for vaporization (water to steam): The heat required for vaporization can be calculated using the formula: Q = m * Lv where Q is the heat required, m is the mass of the water, and Lv is the specific latent heat of vaporization for water. The specific latent heat of vaporization for water is approximately 2260 J/g.
Since the mass of the water formed is equal to the mass of the ice (10g), the heat for vaporization is: Q_vaporization = 10g * 2260 J/g = 22600 J
Therefore, the total heat required to evaporate the water formed is the sum of the heat for melting and the heat for vaporization: Total heat = Q_melting + Q_vaporization Total heat = 3340 J + 22600 J Total heat = 25940 J
So, approximately 25940 J of heat should be supplied to the apparatus to evaporate the water formed.