Final Temperature of Hot Metal in a Calorimeter

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The discussion revolves around calculating the final temperature of a system involving a copper vessel with water and ice, into which a hot lead piece is introduced. The specific heats of copper and lead, along with the melting heat of water, are provided for the calculations. An attempt at solving the problem indicates that the final temperature (T) is small and negative, suggesting that the lead does not completely melt the ice. The user expresses frustration over not being able to delete the thread after realizing the mistake in their calculations. The conversation highlights the complexities of thermal equilibrium in calorimetry problems.
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Homework Statement


A copper vessel of 100 gr contains water, 150 gr, and 8 gr of ice. a 100 gr piece of lead at 2000C is thrown in. what's the final temp'

Homework Equations


Specific heat copper: 0.093
Specific heat lead: 0.031
Melting heat water: 79.7[cal/gr]

The Attempt at a Solution


On the left is the calorie change in the lead:
##100\cdot 0.031(200-T)=(158+100\cdot 0.093)T+8\cdot 79.7##
T comes out small and negative
 
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I solved, it doesn't melt the whole ice, i cannot delete the thread, i don't know how to do it
 

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