25.0 mL of ethanol (density = 0.789 g/mL) initially at 5.5°C is mixed with 32.3 mL of water (density = 1.0 g/mL) initially at 25.3°C in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the mixture?

Answer 1

You will need to look up the specific heat of H2O and the specific heat of ethanol.
heat lost by H2O + heat gained by ethanol = 0
First, use density to convert volumes to grams of each. mass = volume x density
[mass H2O x specific heat H2O x (Tfinal-Tinitial)] + [mass ethanol x specific heat ethanol x (Tfinal-Tinitial)]=0
Substitute and solve for Tfinal.