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ethanol water mixture density

I need chemistry help!?

25.0 mL of ethanol (density = 0.789 g /mL) initially at 7.0 degrees Celsius is mixed with 35.0 mL of water (density = 1.0 g /mL) initially at 25.3 degrees Celsius in an insulated beaker. Assuming that no heat is lost, what is the final temperature of the mixture?

This is simply a weighted average of the combo...but you must realize that the energy content is by weight, not volume.

A. We = 25.0ml x 0.789g/ml = ....g
B. Ww = 35.0ml x 1.00g/ml = ...g

To get the energy content, multiply each by its temp.
C. Ee = A x 7.0*C = ...g*C
D. Ew = B x 25.3*C = ...g*C

Now combine all this
(C + D)g*C / (A + B)g = ...*C

I got 18.7*C...work through it to see if you agree.

Regional Approach, Part 2 of 6 Sustainable Development

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