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 28.0 °C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost to the surroundings?

Use the specific heat capacities of ethanol and water to set up the heat balance equation. The specific heat capacity of ethanol is approximately 2.44 J/g°C and for water, it is 4.18 J/g°C.

Set up the heat balance equation assuming no heat is lost to the surroundings: (mass of ethanol × specific heat of ethanol × (final temperature - initial temperature of ethanol)) + (mass of water × specific heat of water × (final temperature - initial temperature of water)) = 0.