Phase Transitions
If \(8.00 \text{ kg}\) of ice at \(-9.00^\circ\text{C}\) is added to \(25.00 \text{ kg}\) of water at \(40.00^\circ\text{C},\) what is the approximate temperature of the water at equilibrium, assuming that the specific heats of ice and water are \(2220 \text{ J/kg}\cdot\text{K}\) and \(4187 \text{ J/kg}\cdot\text{K},\) respectively and the latent heat of fusion of water is \(3.33 \times 10^5 \text{ J/kg}?\)
If we absorb \(65.0 \text{ kJ}\) of energy from \(650 \text{ g}\) of liquid water at \(0^\circ\text{C},\) approximately how much water remains as liquid state, assuming that the latent heat of fusion of water is \(3.33 \times 10^5 \text{ J/kg}?\)
If \(7.00 \text{ kg}\) of ice at \(0.0^\circ\text{C}\) is added to \(14.00 \text{ kg}\) of water at \(14.0^\circ\text{C},\) approximately how much ice can melt at equilibrium, assuming that the ice-water system is isolated and the specific heat of water is and \(4187 \text{ J/kg}\cdot\text{K},\) and the latent heat of fusion of water is \(3.33 \times 10^5 \text{ J/kg}?\)
If \(70.0 \text{ g}\) of steam at \(100.0^\circ\text{C}\) is mixed with \(350.0 \text{ g}\) of ice at \(0.0^\circ\text{C},\) in a thermally isolated container, what is the approximate temperature of the mixture at equilibrium?
The specific heat of water is \(c_w=4187 \text{ J/kg}\cdot\text{K},\) and the latent heat of fusion and vaporization of water are \(L_f=333 \text{ kJ/kg}\) and \(L_v=2336 \text{ kJ/kg},\) respectively.
How much heat must be absorbed by ice of \(8.00 \text{ kg}\) at \(-17 ^\circ\text{C}\) for the ice to become liquid state water at \(0^\circ\text{C},\) assuming that the specific heat of ice is \(2220 \text{ J/kg}\cdot\text{K}\) and the latent heat of fusion of water is \(3.33 \times 10^5 \text{ J/kg}?\)