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anonymous
 3 years ago
If you have 430.0 mL of water at 25.00 °C and add 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.
anonymous
 3 years ago
If you have 430.0 mL of water at 25.00 °C and add 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.

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anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0I just need help with an equation to use. i've looked over all my notes and can't seem to come up with anything. I don't really want an answer, more of a bit of help.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0you will also need heat capacity of water... and then you go with this equation: Q = m * cp * (T2T1) where Q = heat m = mass cp = heat capacity of water (T2T1) = temperature now since you have heating of colder water and cooling of hotter water you write: Q(hot) =  Q(cold) and T2 is your final temperature on both sides so you have: m(h) * cp(w) * (T2  95) = m(c) * cp(w) * (T2  25) where indexes are: h  hot c  cold w  water and all you need to do is to solve that equation for T2 and you will get your answer! hope this helps ;)
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