David Sang and Darrell Hamilton Solutions for Chapter: Thermal Properties of Matter, Exercise 5: Exercise 10.4

State which of the metals shown in the table will require the greatest amount of energy to raise the temperature of $100 \mathrm{g}$ from room temperature to $200 °\mathrm{C}$. 

You have two identical glass beakers containing equal amounts of water and seawater. You heat them using identical electrical heaters, and record their temperatures as they rise. State which temperature will rise more quickly. Explain your answer.

A $1.0 \mathrm{kg}$ block of steel is heated in an oven to a temperature of$200 °\mathrm{C}$. It is then dropped into a tank containing $100 \mathrm{kg}$ of water. The experiment is then repeated using a $1.0 \mathrm{kg}$ block of aluminium. State which metal block will cause a bigger rise in the temperature of the water. Explain your answer. 

All metals have a lower specific heat capacity than all non-metals.

Metals generally have a higher specific heat capacity than non-metals.

The specific heat capacity of water decreases when it freezes.

The specific heat capacity of water decreases when it boils.

If the temperature rise of $1000 \mathrm{kg}$ of water had to be limited to $80 °\mathrm{C}$, calculate how much energy it could store if its specific heat capacity is $4200 \mathrm{J}/ \mathrm{kg}°\mathrm{C}$.