Apiece of unknown material of mass 0.15 kg is heated to 114°c without melting and then placed in a calorimeter containing 0.74 kg of water initially at 14.9°c. the system reaches an equilibrium temperature of 20.2°c. what is the specific heat of the unknown material, in units of j (kg·°c)? the specific heat of water is 4.186 x 103 j (kg·℃

To perform this exercise it is necessary to use the theory of the first Law of Thermodynamics, in relation to Heat Capacity. If one adds heat to an object, its temperature usually increases (exceptions include at a state boundary, for example when a liquid boils). In many cases the temperature change is linear in the amount of heat added. We define the heat capacity C of an object from the relation:

Where

Heat that flows into system

Temperature

c = Specific heat

m = Mass

From our values we have the exchange of heat of the material and of the water, that is,

For the water:

Where,

For the Material:

Where,

For conservation of energy in balance we have to,

neither accurate nor precise.

the answer is the first electromagnet (a). this is because it has more coils around the ferromagnetic material. increasing the number of coils increases the surface area in which the metal interacts with the current in the coil. this enables more atoms in the metal to become aligned hence becoming more magnetized.