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When 155 mL of water at 26 C is mixed with 75 mL of water at 85 C, what is the final temperature? (Assume that no heat is lost to the surroundings; d of water 1.00 g/mL.)
 one year ago
 one year ago
When 155 mL of water at 26 C is mixed with 75 mL of water at 85 C, what is the final temperature? (Assume that no heat is lost to the surroundings; d of water 1.00 g/mL.)
 one year ago
 one year ago

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pnicoleBest ResponseYou've already chosen the best response.0
Someone please help, I really don't know where to begin or how to solve this. :( Even just an equation will do.
 one year ago

wachBest ResponseYou've already chosen the best response.0
I'm not that familiar with this exact calculation, so excuse me if I'm wrong. The equation for this should be : ( Volume1 * Temp1) + (Volume2 * Temp2) / (Volume1 + Volume2) = Final temp
 one year ago

NoelGrecoBest ResponseYou've already chosen the best response.1
The amount of heat a substance gains or loses is governed by the following formula: \[Q=mc \Delta T\] Where Q is the heat lost or gained, m is the mass in kg, c is the specific heat of the substance (c1.00 for water), and deltaT is the change in temperature. Since the heat gained by the cold water is = to the heat lost by the warm water the two Qs can are equal. Thertefore: \[m _{c} \Delta T _{c }=m _{w}\Delta T _{w}\] The c and w subscripts are for the cold and warm water. Since both waters are at the same final temperature: \[m _{c}(T _{f}26)=m _{w}(85T _{f})\] where T sub f is the final temp for both masses of water. The expressions in the parentheses were switched because you always want a positive delta T.
 one year ago
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