A system consists of a 0.130-kg chunk of ice floating in 1.12 kg of water, all at 0 ∘C.?
How much thermal energy must be added to the system to convert it to 1.25 kg of water at 15.0 ∘C?
Hey guys. I am very confused. Could you help me set this up. Someone answered this
= heat required to melt .130 kg ice+heat required to raise temperature of 1.25 kg of water from 0 to 15
But I still don't understand. Thanks
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in other words, all the ice has to be melted. The water is already at 0º as is the ice, so all we need is:
heat of fusion of ice is 334 kJ/kg
energy = 0.13 kg x 334 kJ/kg = 43.42 kJ
now we have to warm all of the 1.25 kg of water 15º
specific heat of water is 4.186 kJ/kgC = 4.186 J/gC
E = 1.25 kg x 4.186 kJ/kgC x 15ºC = 78.49 kJ
total is the sum = 121.9 kJ