- #1
majormuss
- 124
- 4
Homework Statement
An 11 g ice cube at -16.0˚C is put into a Thermos flask containing 120 cm3 of water at 24.0˚C. By how much has the entropy of the cube-water system changed when a final equilibrium state is reached? The specific heat of ice is 2200 J/kg K and that of liquid water is 4187 J/kg K. The heat of fusion of water is 333 × 103 J/kg.
Homework Equations
The Attempt at a Solution
I desperately need help.. I keep solving for almost one hour and my answers is surely wrong. I approached it by solving Q1 for the ice to heat up from -16C to 0, then melts, then comes to a final temperature, then i can use that to find entropy change.. but my final temperature camee out to be 36C- that is impossible.. pls help
these are my numbers to find the final temperature
FOR ICE ------------------------- FOR WATER
Q1= 387.2 J -------------------------468.944(T-final -24)
Q2= 3663 J
Q3=46.1(T- final)
my resulting answer is nonsensical! was my approach wrong? what is the best procedure?