Posted by **Lindsay** on Tuesday, May 15, 2007 at 5:04pm.

A 63 gram block of an unknown metal at 88 degrees C was dropped into an insulated flask containing approx. 30 g of ice and 30 g of water at 0 degrees C. After the system had reached a steady temp. it was determined that 12.1 g of ice had melted. What is the specific heat of the metal?

Ok so I know that this problem involves the specific heat equation: q= mass x constant x change in temp. And I know that the heat of fusion of ice is 333 J/g. But I'm not sure of how to rearrange this equation or where to plug in the numbers.

If all the ice did not melt, there was no change in temperature.

Heat change= massicemelted*Heatfusionice

I guess I still don't really understand...

Bob Pursley is saying that a mixture of ice and water at zero degrees C will stay at that temperature until all of the ice is melted. If you had ice left after the experiment was performed, the final T of the ice/water mixture must still be zero degrees C. Thus the unknown metal melted ice (at 334 J/g) but it didn't raise the T of the mixture. (Therefore, you don't have a delta T)

Ok I see. But he said that heat change = the mass of the ice melted x the heat of fusion. Once I come up with this number, what would the next step be?

Do I have to rearrange the specific heat equation?

Ahh n/m ok I got it. :)

What answer did you obtain?

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