An insulated beaker with negligible mass contains liquid water with a mass of 0.230 kg and a temperature of 72.0 ∘C .
How much ice at a temperature of -13.8 ∘C must be dropped into the water so that the final temperature of the system will be 20.0 ∘C ?
Take the specific heat of liquid water to be 4190 J/kg⋅K , the specific heat of ice to be 2100 J/kg⋅K , and the heat of fusion for water to be 3.34×105 J/kg .
The unknown mass of ice is M.
Q(heat energy)=(mass)(specific heat)(delta T)
The amount of heat lost by the 0.230 kg of water in the beaker to the ice is easily calculated:
Q(beaker liquid) = (0.230)x(4190)x(72-20) = 50112.4 joules
The amount of heat gained by the ice will be:
Q(ice) + Q(fusion) + Q(liquid) for the unknown mass M
Heat lost by beaker liquid = Heat gained by ice when equilibrium is reached.
50112.4 = (28980)M + (3.34x10^5)M + (83800)M
50112.4 = (28980 + 3.34x10^5 + 83800)M
50112.4 = (446780)M
50112.4/446780 = M
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