Classical Mechanics

Phase Transitions

Phase changes

         

If 8.00 kg8.00 \text{ kg} of ice at 9.00C-9.00^\circ\text{C} is added to 25.00 kg25.00 \text{ kg} of water at 40.00C,40.00^\circ\text{C}, what is the approximate temperature of the water at equilibrium, assuming that the specific heats of ice and water are 2220 J/kgK2220 \text{ J/kg}\cdot\text{K} and 4187 J/kgK,4187 \text{ J/kg}\cdot\text{K}, respectively and the latent heat of fusion of water is 3.33×105 J/kg?3.33 \times 10^5 \text{ J/kg}?

If we absorb 65.0 kJ65.0 \text{ kJ} of energy from 650 g650 \text{ g} of liquid water at 0C,0^\circ\text{C}, approximately how much water remains as liquid state, assuming that the latent heat of fusion of water is 3.33×105 J/kg?3.33 \times 10^5 \text{ J/kg}?

If 7.00 kg7.00 \text{ kg} of ice at 0.0C0.0^\circ\text{C} is added to 14.00 kg14.00 \text{ kg} of water at 14.0C,14.0^\circ\text{C}, approximately how much ice can melt at equilibrium, assuming that the ice-water system is isolated and the specific heat of water is and 4187 J/kgK,4187 \text{ J/kg}\cdot\text{K}, and the latent heat of fusion of water is 3.33×105 J/kg?3.33 \times 10^5 \text{ J/kg}?

If 70.0 g70.0 \text{ g} of steam at 100.0C100.0^\circ\text{C} is mixed with 350.0 g350.0 \text{ g} of ice at 0.0C,0.0^\circ\text{C}, in a thermally isolated container, what is the approximate temperature of the mixture at equilibrium?

The specific heat of water is cw=4187 J/kgK,c_w=4187 \text{ J/kg}\cdot\text{K}, and the latent heat of fusion and vaporization of water are Lf=333 kJ/kgL_f=333 \text{ kJ/kg} and Lv=2336 kJ/kg,L_v=2336 \text{ kJ/kg}, respectively.

How much heat must be absorbed by ice of 8.00 kg8.00 \text{ kg} at 17C-17 ^\circ\text{C} for the ice to become liquid state water at 0C,0^\circ\text{C}, assuming that the specific heat of ice is 2220 J/kgK2220 \text{ J/kg}\cdot\text{K} and the latent heat of fusion of water is 3.33×105 J/kg?3.33 \times 10^5 \text{ J/kg}?

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