 Classical Mechanics

# Phase changes

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 $3.33 \times 10^5 \text{ J/kg}?$

×