[mass ice x heat fusion]+[mass melted ice x specific heat ice x (Tfinal-Tinitial)] + [mass warm water x specific heat H2O x (Tfinal-Tinitial)] = 0
Substitute the numbers and solve for Tf.
What amount of energy is required to melt a 27.4 g piece of ice at 0oC?
The heat of fusion of ice = 333 Jg-1
Heat required to melt the ice 9.12e3 = J
What amount of energy must be removed from 123 g of water to cool it from 71.6oC to 9.41oC?
Specific heat of water = 4.184 JK-1g-1
Enter the heat as a negative amount (heat removed from a system is by convention always negative).
Heat removed to cool the water =-3.2e4 J
What is the final temperature after a 27.4 g piece of ice is placed into a styrofoam cup containing 123 g of hot water at 71.6oC. The mass of the ice, and the mass and initial temperature of the hot water are the same as in the two previous parts of this question.
Final temperature = oC
I got the first two answers I just don't know how to find the answer to the last questions.
1 answer
1 answer