The specific heat of ice is $2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}$, the heat of fusion for ice at $0{ }^{\circ} \mathrm{C}$ is $333.7 \mathrm{~kJ} / \mathrm{kg}$, the specific heat of water $4.186 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}$, and the heat of vaporization of water at $100^{\circ} \mathrm{C}$ is $2,256 \mathrm{~kJ} / \mathrm{kg}$. What is the final equilibrium temperature when 10.0 grams of ice at $-15.0^{\circ} \mathrm{C}$ is mixed with 3.00 grams of steam at $100^{\circ} \mathrm{C}$ ?

Question

Quizplus · Accepted Answer

The heat gained by the ice as it warms to 0°C, melts, and then warms to the final temperature is equal to the heat lost by the steam as it condenses and cools to the final temperature. Calculating these heat exchanges and setting them equal allows us to solve for the final temperature, which is $80.3^{\circ} \mathrm{C}$.

The Specific Heat of Ice Is 2.10 kJ/kg∘C2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}2.10 kJ/kg∘C

The Specific Heat of Ice Is $2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}$