Question

How do specific heats of metal compare to that of water?

Answer 1

The basic hint here we have the keyword specific heats of metal and water. The specific heats of the metals are being usually less than one and these are less than of water which is around $4.18\text{ }\dfrac{J}{gC~}$ Therefore we now that the specific heat is amount of a heat energy needed to raise temperature by the $1$ degree Celsius for a $1gram$ of substance.

Complete step-by-step answer: The key concept here is specific heat and specific heat of metals are way lower than the Specific heat of water.
Specific heat capacity is measurement how much energy in J could have to be added to a $1Kg$ of the substance which has to increase material temperatures of the given substance by $1{}^\circ C$ So our substance with given or specified low specific heat capacity heat up more vastly thus, by then the object or substance can lose their heat vigorously. Substances with a high specific heat capacity require a larger amount of heat that could be added to the change in these temperatures by which these all have their heat much wider and longer.
Example:
Liquid water $4.18\text{ }\dfrac{J}{gC~}$
Aluminum $\text{0}\text{.897 }\dfrac{J}{gC~}$
Lead $\text{0}\text{.129 }\dfrac{J}{gC~}$
Titanium $0.523\text{ }\dfrac{J}{gC~}$
From these above values, we can easily determine that it took much less energy to raise the temperature of metal than it does for the water; this clearly states the water and metal variation with Specific heat.

Note: Note that the specific heat of metals is lower than that of water. Substances with a high specific heat capacity require a large amount of heat to be added to change their temperature but then they hold their heat much longer.