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BlueSkyy
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Melting Ice With Aluminum??
How many grams of aluminum at 90 degrees C would have to be dropped into a hole in a block of ice at 0.0 degrees C to melt 10 g of ice?
Q = (m)(c)(deltaT)
c of aluminum = 0.9
c of ice = 2.1
c of water = 4.186
333.7 kJ is needed to get past the ice/water boundary
I've tried setting up a few different equations, like:
(.01 kg)(2.1)(+45) + (x kg)(0.9)(-45) = 0
(.01 kg)(2.1)(+45) + 333.7 + (x kg)(0.9)(-45) = 0
and a few others I don't have on hand, but I can't seem to get the correct answer. What do I use for delta T? Am I even doing this right at all?
Thanks for your help.
Homework Statement
How many grams of aluminum at 90 degrees C would have to be dropped into a hole in a block of ice at 0.0 degrees C to melt 10 g of ice?
Homework Equations
Q = (m)(c)(deltaT)
c of aluminum = 0.9
c of ice = 2.1
c of water = 4.186
333.7 kJ is needed to get past the ice/water boundary
The Attempt at a Solution
I've tried setting up a few different equations, like:
(.01 kg)(2.1)(+45) + (x kg)(0.9)(-45) = 0
(.01 kg)(2.1)(+45) + 333.7 + (x kg)(0.9)(-45) = 0
and a few others I don't have on hand, but I can't seem to get the correct answer. What do I use for delta T? Am I even doing this right at all?
Thanks for your help.