Suppose a piece of metal at 90 °C is quickly transferred into a Styrofoam cup containing 212 grams of water at 24 °C. After a minute or so, the temperature of the contents of the cup is stable at 35 °C. Use 4.2 J/(g•°C) as the specific heat capacity of water and assume that during this time the energy transferred between the contents of the cup and the surroundings is negligible and that there is no heat loss to the cup. (a) How much heat in joules is gained by the water? (b) How much heat in joules is lost by the metal? (c) What is the heat capacity of this piece of metal? (d) If the mass of the metal is 196 grams, what is its specific heat capacity? (e) What is the change of water's entropy? Note the volume of water stays the same. (f) What is the change of total entropy of the system, including both water and metal?
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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