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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.
 one year ago
 one year 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.
 one year ago
 one year ago

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afa92Best ResponseYou've already chosen the best response.0
I 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.
 one year ago

KrytenBest ResponseYou've already chosen the best response.0
you 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 ;)
 one year ago
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