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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).

  1. 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

  1. 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.

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