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PhysicsInNJ
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Homework Statement
A 3.60 kg block of copper at a temperature of 92 °C is dropped into a bucket containing a mixture of ice and water whose total mass is 1.50 kg. When thermal equilibrium is reached the temperature of the water is 5 °C. How much ice was in the bucket before the copper block was placed in it?
(ci = 2000 J/(kg.°C), cw = 4186 J/(kg.°C), Lf=3.35 × 105 J/kg, Lv=2.26 × 106 J/kg, ccopper = 387 J/(kg.°C). Neglect the heat capacity of the bucket.)
Homework Equations
Q=mcΔT
Q=mL
The Attempt at a Solution
Because of conservation of heat, the energy the copper block loses must be gained by the ice/water system.
So; QLOST= QGAINED
Expanded it should become something like;
(cmΔT)COPPER =
(heat to raise temperature of ice) + (heat to raise temperature of water) + (latent heat to melt ice) + (latent heat to vaporize water)
However I think there are too many unknowns at this point.
Any idea on what a possible next step could be / look like, or if I'm even doing this remotely correctly?
All help appreciated!