2.997 kg of ice at -35 degrees Celsius are thoroughly mixed with 138.6 kg of water at 3.9 degrees Celsius in a well-insulated container at standard temperature and pressure.
Determine the proportions of ice (if any) and water in the final mixture.
Bonus: what is being simulated?
With specific heat of ice at 2.108 kJ/kg-K (or C), water 4.187 kJ/kg-K, and heat of fusion of 334 kJ/kg
Warming the ice to 0deg C = 2.997*2.108*35=221.118 kJ
Melting the ice @ 0 C to water @ 0C = 2.997*334=1000.998 kJ
Cooling the initially liquid water to 0deg = 138.6*4.187*3.9 =2263.242 kJ
So the ice melts completely. Going through the algebra, I get a final state of of 141.597 kg of liquid water at 1.758 C
I have no idea what this represents, but a wild guess, based on the 3.9C initial water temperature may have something to do with ice having less density than water at around 4 C? How this is related to the problem I can't guess.
Edited on April 28, 2013, 10:25 am
Edited on April 28, 2013, 10:26 am
Edited on April 28, 2013, 10:28 am
Posted by Kenny M
on 2013-04-28 10:25:13