chemistry question

Question

If you combine  of water at  and  of water at  what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

Tfinal= ___∘C

Answer 1

Heat lost by hot water = heat gained by cold water

heat = m x C x ∆T where m = mass; C = specific heat; ∆T = change in temperature

Since density of water is 1.00 g/ml, the mls of water = grams of water.

Specific heat of water = 4.184 J/g/degree

Heat lost by hot water = heat gained by cold water

(110 g)(4.184 J/g/deg)(95º - Tf) = (290 g)(4.184 J/g/deg)(Tf - 25º) and you can cancel 4.184 from each side...

10,450 - 110Tf = 290Tf - 7250

400Tf = 17,700

Tf = 44.25ºC