posted by Elle .
25.0 mL of ethanol (density = 0.789 g/mL) initially at 7.0 degrees celsius is mixed with 35.0 mL of water (density = 1.0 g/mL) initially at 25.3 degrees celsius in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the mixture?
Use density to convert mL ethanol to grams.
Use density to convert mL H2O to grams.
heat gained by ethanol + heat lost by H2O = 0
[mass ethanol x specific heat ethanol x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
Substitute and solve for Tfinal.