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anonymous
 3 years 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.)
anonymous
 3 years 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.)

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

wach
 3 years ago
Best ResponseYou've already chosen the best response.0I'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

NoelGreco
 3 years ago
Best ResponseYou've already chosen the best response.1The 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.
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