Question

Problem #3 A container is filled with a mass m of water at room temperature T, (specific heat c,' latent heat of vaporization L, density at room temperature p, coefficient of volume expansion B). A very hot mass m2 of copper (specific heat c2) is put into the water and when equilibrium is reached half the water has evaporated. Assume that there is no significant exchange of heat with the suroundings. (note: T-0°C, T100-100°C) a) What is the initial volume of water? b) Calculate the initial temperature of the copper. c) How much heat is transferred from the copper to the water? d) What is the final volume of water? Make sure to write your results only as function of input parameters!

Answer 1

Let initial volume of water be volame = ame = mass Jensity - During the process, water temperature first increases to boiling point Too and then it starts to evaporate. - Let T be the initial temperature of copper: - Since the water gets evaporated and only half of water gets evaporated we can say that final equilibrium temperature is Too. So, heat transferred from copper to water can be found by formula 10 = MC AT /

Here, it is Q = m_ c, (1, - Tou). read - This heat is used to increase temperature of water and evaporate it. - heat used to increase temperature is Q = m, g (Two-T) - heat used to evaporate the water B half Q,= (m.) :- Since, no heat is exchanged with surroundings, Q=Q,+Q, m, Ca (Ta-Tom) = m,c. (1-2) + m2

Ty-Too time (T-1) + So; initial temperature of copper mc T he Crow - 7) + can contro (C) Heat transferred from copper to water is a= mica (7.-Too) which is = mg, (Two-T.) + ML (1) Final mass of water is mer final density is s's Tecm-1) final volume = MCI+PCT.-)) 201 - 29