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25.0 mL of ethanol (density = 0.789 g/mL) initially at 4.2°C is mixed with 35.7 mL of water (density = 1.0 g/mL) initially at 2...Asked by Lisa
25.6mL of ethanol (density =0.789 g/mL) initially at 5.4∘C is mixed with 30.4mL of water (density = 1.0 g/mL) initially at 20.4∘C in an insulated beaker.Assuming that no heat is lost, what is the final temperature of the mixture?
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Answered by
DrBob222
heat gained by water + heat lost by ethanol = 0
[mass H2O x specific heat H2O x (Tfinal-Tinitial)] + [mass ethanol x specific heat ethanol x (Tfinal-Tinitial)] = 0.
You will look up the specific heats ethanol and H2O.
[mass H2O x specific heat H2O x (Tfinal-Tinitial)] + [mass ethanol x specific heat ethanol x (Tfinal-Tinitial)] = 0.
You will look up the specific heats ethanol and H2O.
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