Asked by MD
                25.6 {\rm mL} of ethanol (density =0.789 {\rm g}/{\rm mL}) initially at 8.0^\circ {\rm C} is mixed with 39.5 {\rm mL} of water (density = 1.0 {\rm g}/{\rm mL}) initially at 23.1^\circ {\rm C} in an insulated beaker.
Assuming that no heat is lost, what is the final temperature of the mixture?
            
        Assuming that no heat is lost, what is the final temperature of the mixture?
Answers
                    Answered by
            DrBob222
            
    [mass ethanol x specific heat ethanol x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
The only unknown is Tf. Solve for that.
    
The only unknown is Tf. Solve for that.
                    Answered by
            MD
            
    so am I treating density as Sp. heat? 
    
                    Answered by
            DrBob222
            
    Of course not. Use density  as in mass = volume x density to convert the volumes in the problem to grams. The specific heat is either given in the problem or it will be in your text/notes. I don't have specific heat tables memorized although I remember that H2O is 4.184 J/g*C or 1 cal/g*C. Use the one you are familiar with. 
    
                                                    There are no AI answers yet. The ability to request AI answers is coming soon!
                                            
                Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.