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
Achieve wk 3/4 #9
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Re: Achieve wk 3/4 #9
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
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
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Re: Achieve wk 3/4 #9
here is the equation i used!
350 g * 4.18 J/gK *(Tf-25)=140 g * 4.18 J/gK *(Tf-95)
350 g * 4.18 J/gK *(Tf-25)=140 g * 4.18 J/gK *(Tf-95)
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Re: Achieve wk 3/4 #9
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!
(440g)(4.184J/g*C)(F-25) = -(130g)(4.184J/g*C)(F-95)
Hope this helps!
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