29.8 ml of ethanol (density = 0.789 g/ ml) initially at 9.9 degree celsius is mixed with 33.8 mL of water (density = 1.0 g/mL) initially at 27.8 degree celcius in an insulated beaker. Assuming that no heat is lost, what is the final temperature of mixture?

Question

29.8 ml of ethanol (density = 0.789 g/ ml) initially at 9.9 degree celsius is mixed with 33.8 mL of water (density = 1.0 g/mL) initially at 27.8 degree celcius in an insulated beaker. Assuming that no heat is lost, what is the final temperature of mixture? 
How do I start this problem?

DrBob222 · Answer

heat gained by ethanol + heat lost by water = 0
heat gained by ethanol = mass x specific heat x (Tfinal-Tinitial). Use density to convert mL to mass.

heat lost by water = mass x specific heat x (Tfinal-Tinitial). Use density to convert mL to mass.
Tfinal is the only unknown.