If 45.0 ml of ethanol (density=0.789 g/ml) initially at 9.0 c is mixed with 45.0 ml of water (density=1.0 g/ml) initially at 28.6 c in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?

i tried many times in trying to get the answer, but i keep getting it wrong. i appreciate who answers this writes it step by step. you.

Answer : The final temperature of the mixture is

Explanation :

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

And as we know that,

Mass = Density × Volume

Thus, the formula becomes,

where,

= specific heat of ethanol =

= specific heat of water =

= mass of ethanol

= mass of water

= density of ethanol = 0.789 g/mL

= density of water = 1.0 g/mL

= volume of ethanol = 45.0 mL

= volume of water = 45.0 mL

= final temperature of mixture = ?

= initial temperature of ethanol =

= initial temperature of water =

Now put all the given values in the above formula, we get

Therefore, the final temperature of the mixture is

43.452

step-by-step explanation:

284 times .153 = 43.452

answer: you could do some invislibe ink.

explanation: i will tell you how to if u answer my question.