Question

Heat is added to ice initially at $0^{\circ}C$ until the ice changes completely into the water. The same amount of heat continues to be added to the liquid water for $15\;mins$. Identify which of the following statements are true?

Answer 1

We know that heat is a form of energy which can be transferred from one system to another. We also know that temperature is the measure of heat energy possessed by the system. However, the concept of hot and cold is relative in nature. Also, heat energy generally flows from the hot body to a cold body in nature; the reverse may require extra effort.

Complete step-by-step solution: -
The study of heat energy or temperature and its constituents is called thermodynamics. The heat energy often is used to change the phase of the substance depending on the nature of the bonds which exist between the substances but the temperature of the system remains the same. Such energies are called latent heat.
For example, the conversion of water to steam at $100^{\circ}C$, here both the water and steam exist in equilibrium, and is called latent heat of vaporization . Similarly, in the conversion of ice to water at $0^{\circ}C$, here both ice and water exist in equilibrium and are called the latent heat of melting.
Any further increase in heat, increases the temperature of the system.
Thus we can say that in the given question, after the ice melts into water in the next $15\;mins$, the temperature of the system increases.

Note: There are systems called isothermal systems , where there is no loss in heat energy since the boundary of the system is insulated. An example of such a system is the thermos flask, where the substance in the thermos flask remains hot or cold irrespective of the temperature outside the flask.