# Problem: 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 28.5˚C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost? (CEtOH= 2.42 J/(g•C), cwater = 4.18  J/(g•C))

###### FREE Expert Solution

Recall that heat can be calculated using the following equation:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{∆}}{\mathbf{T}}}$

+qabsorbs heat
–qloses heat

heat transfer: hot to cold

Since there is no heat lost to the surroundings:

heat lost by water = heat absorbed by ethanol

– qCu = + qwater

At thermal equilibrium:

▪ final temperature of ethanol = final temperature of water = final temperature of system

###### Problem Details

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 28.5˚C in an insulated beaker, what is the final temperature of the mixture, assuming that no heat is lost? (CEtOH= 2.42 J/(g•C), cwater = 4.18  J/(g•C))