Achieve wk 3/4 #9

[Kaethe Zappacosta 2L]

If you combine 350.0 mL of water at 25.00 ∘C and 140.0 mL of water at 95.00 ∘C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

I am confused because we don't know delta T and we don't know delta H. I don't really know where to start

[Caroline 2A]

Hi!

The equation you will use is q=mc(deltaT). Then all you need to do is solve for the different temperatures after.

Hope this helps

[Selene_Lam_1G]

here is the equation i used!

350 g * 4.18 J/gK *(Tf-25)=140 g * 4.18 J/gK *(Tf-95)

[Ryan Khiev 1L]

To solve for this problem, you set two values of q equal to each other. Since one of the samples (130g) is at a higher initial temperature, that means its q value should be negative, because it's giving away its heat. Since the other (440g) is at a lower initial temperature, it absorbs heat from the other sample, and its q value is positive. Then you can set up the following equation and solve for F, which is the final temperature:

(440g)(4.184J/g*C)(F-25) = -(130g)(4.184J/g*C)(F-95)

Hope this helps!