Posted by anthony on Wednesday, April 11, 2012 at 2:05am.
0 degree celcius because all the ice has not melted or 4 degree celcius.
For the ice to reach 0 degrees, you will need Q = c• m• ΔT 0.04• 2090 • 71 = 5935,6 J
The latent heat needed to melt the ice is 334 000 J / kg.
So to melt the ice, you will need 334 000 • 0.040 = 13360 J
Assume final temperature = x degC
Specific heat of water is 4180 J / k g degC.
So heat applied to ice will be 0.04• 4180• x = 1672 x
Total heat energy applied = 5935,6 + 13360 + 167,2x
Heat from water =0.590 • 4180 • (27-x) = 2466.2• (27-x)
Specific heat of copper is 385 J / kg degC.
Heat from copper = 0.08• 385 • (27-x) = 30.8• (27-x)
Heat gained = heat loss
5935,6 + 13360+167.2 x =2466.2(27-x) +30.8• (27-x)
19296 +167.2 x = 2466.2• (27-x) +30.8• (27-x)
x =8.53
So final temperature is 8.53 degC.
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