Sixty-five liters of liquid ethanol at 70.0 derajat celcius and 55 L of liquid water at 20.0 derajat celcius are to be mixed in a well-insulated flask. The energy balance for this constant pressure process is Q=ΔH.
a) Neglecting evaporation and the heat of mixing, estimate the final mixture temperature. b) If the experiment were actually performed and the final mixture temperature were measured, it would almost certainly not equal the value estimated in Part (a). List as many reasons as you can to explain the observation. (there are at least seven of them, most involving approximations made in the estimation.)

The temperature that is required is 44.3 celcius in the Sixty-five liters of liquid ethanol at 70.0 celcius and 55 L of liquid water at 20.0.

Here we have the 75 L of ethanol;

789 * 1 mol /46.07 = 1284 mol of ethanol.
Heat required = Q= 4H = mT1/T2
Q =4U=4H
T=44.3 celsius.
Mixing the solution may have an effect on the very last temperature.
Heat loss to the outdoor of the system (now no longer adiabatic)
Evaporation of the drinks will have an effect on the very last temperature.
Heat capability of water won't be constant.
There wherein each systematic and random mistakess that came about at some stage in the test along with errors in size of temperatures and volume. It also can be the shortage of accuracy and precision of the researcher.