CA-2 Suppose you have 2.00 kg of liquid water at a temperature of 20.0°C. You also have a large supply of ice cubes which are stored at a temperature of –20.0°C. The specific heat of solid ice is 2108 J kg-1 °C-1, the latent heat of fusion of water is 333,500 J kg-l, and the specific heat of liquid water is 4186 J kg-1 °C-1. (a) What is the maximum mass of ice you can mix with the liquid water so that all of the ice melts once thermal equilibrium is reached? Assume no heat is lost from the ice + liquid water system during the process. (b) Suppose you add twice the mass of ice that you found in part a. How much solid ice will remain once thermal equilibrium is reached? Hint: the final state will be a mixture of liquid water and solid ice.
Energy transfer
The flow of energy from one region to another region is referred to as energy transfer. Since energy is quantitative; it must be transferred to a body or a material to work or to heat the system.
Molar Specific Heat
Heat capacity is the amount of heat energy absorbed or released by a chemical substance per the change in temperature of that substance. The change in heat is also called enthalpy. The SI unit of heat capacity is Joules per Kelvin, which is (J K-1)
Thermal Properties of Matter
Thermal energy is described as one of the form of heat energy which flows from one body of higher temperature to the other with the lower temperature when these two bodies are placed in contact to each other. Heat is described as the form of energy which is transferred between the two systems or in between the systems and their surrounding by the virtue of difference in temperature. Calorimetry is that branch of science which helps in measuring the changes which are taking place in the heat energy of a given body.
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