State the minimum possible temperature on the Celsius scale and on the Kelvin scale.
As the solid's temperature rises, it is still a solid. Describe how the motion of the particles changes.
The solid melts. State what happens to the internal energy and the temperature of the solid while it melts.
A student puts a $300\,\text{g}$ block of iron into boiling water until it reaches $100\,^{\circ}\text{C}$. The iron is then taken out and placed immediately into $100\,\text{g}$ of water at $25\,^{\circ}\text{C}$. The iron cools while the water warms, and both end up at the same temperature, $44\,^{\circ}\text{C}$. The specific heat capacity of water is $4.2\,\text{J (g }^{\circ}\text{C)}^{-1}$. No energy is lost to the surroundings. Calculate the change in energy (internal energy) of the water as it warms up.
Calculate the specific heat capacity of iron.