Heat Capacity and Specific Heat Capacity

If objects of equal masses are given equal heat, their final temperature will be different. This is due to difference in their :

The specific heat capacity of water is less than that of steam.

The specific heat capacity of water is less than that of ice.

A cube of lead of $500 \mathrm{g}$ at $25 °\mathrm{C}$ is supplied with a $3225 \mathrm{J}$ heat. Find the final temperature (in degree Celsius) of the lead cube. (Take, specific heat of lead is $0.129 \raisebox{1ex}{$\mathrm{J}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{g} °\mathrm{C}$}\right.$) 

Calculate the heat energy (in joules) to raise the temperature of $5 \mathrm{kg}$ of water from $20 °\mathrm{C}$ to $100 °\mathrm{C}$. (Take specific heat of water, $s_w=4.2\times {10}^3 \mathrm{J} {\mathrm{kg}}^{-1} {\mathrm{K}}^{-1}$)

Which material would cool down the fastest when removed from heat?

What property of water helps stabilize body temperature?

Why is copper used in cookware despite its low specific heat capacity?

What is the temperature change if 100 J of heat is added to a 2 kg substance with a specific heat capacity of 10 J/kg·K?

What is the main reason for using water in car radiators?

How does the specific heat capacity of metals compare to non-metals?

Which physical state generally has the highest specific heat capacity?

What happens to heat capacity when the mass of an object doubles?

Which device measures specific heat capacity experimentally?

Why does sand heat up faster than water under the sun?

How does specific heat capacity affect climate near oceans?

Which equation relates heat energy, mass, specific heat capacity, and temperature change?

What does a high specific heat capacity imply about a substance?

What is the heat capacity of an object if 2000 J of energy raises its temperature by 10 K?

Why does water take longer to heat up compared to iron?