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Category > Physics Posted 08 Jul 2017 My Price 5.00

No heat is lost to the surroundings

.Suppose that 206 g of ice at 0.0oC is mixed with 648 g of water. What should be the initial temperature of the water if the ice is to just melt completely, leaving only water at 0.0oC? Assume that no heat is lost to the surroundings. answer in Celsius

 

HINT:No heat is lost to the surroundings, so the magnitude of heat Qhot that flows from the water is equal to the magnitude of heat Qcold that flows into the ice—that is, Qcold=Qhot (Equation 13.3.2). The ice experiences a phase change as it melts. The water simply cools down to its freezing temperature. Using Q=mcΔT

for the temperature change and Q=mLf for the phase change, Qcold=Qhot

can be written as

(m'Lf)=(mc|ΔT|)

(ice melts) = (water cools)

m′ is the initial mass of ice and m is the initial mass of water. Solve for |ΔT|, from which the initial temperature of the water may be deduced.

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SuperTutor
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Status NEW Posted 08 Jul 2017 02:07 AM My Price 5.00

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