Asked by tanner
What amount of energy is required to melt a 26.9 g piece of ice at 0oC?
The heat of fusion of ice = 333 Jg-1
Heat required to melt the ice = J
What amount of energy must be removed from 120 g of water to cool it from 72.1oC to 12.4oC?
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 = J
What is the final temperature after a 26.9 g piece of ice is placed into a styrofoam cup containing 120 g of hot water at 72.1oC. 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 =
The heat of fusion of ice = 333 Jg-1
Heat required to melt the ice = J
What amount of energy must be removed from 120 g of water to cool it from 72.1oC to 12.4oC?
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 = J
What is the final temperature after a 26.9 g piece of ice is placed into a styrofoam cup containing 120 g of hot water at 72.1oC. 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 =
Answers
Answered by
DrBob222
#1. mass ice x deltaHfusion = ?
#2. q = mass x specific heat x (Tfinal-Tinitial) = ?
#3.
You can put the pieces together.
heat to melt ice + heat to raise T of melt from zero C to final T + heat lost by hot water going to lower final T.
#2. q = mass x specific heat x (Tfinal-Tinitial) = ?
#3.
You can put the pieces together.
heat to melt ice + heat to raise T of melt from zero C to final T + heat lost by hot water going to lower final T.
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