Recall that heat can be calculated using the following equation:
• +q → absorbs heat
• –q → loses heat
heat transfer: hot to cold
Since there is no heat lost to the surroundings:
heat lost by water = heat absorbed by ethanol
– qCu = + qwater
At thermal equilibrium:
▪ final temperature of ethanol = final temperature of water = final temperature of system
If 55.0 mL of ethanol (density = 0.789 g/mL) initially at 8.0˚C is mixed with 55.0 mL of water (density = 1.0 g/mL) initially at 28.5˚C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost? (CEtOH= 2.42 J/(g•C), cwater = 4.18 J/(g•C))
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