The discussion revolves around determining the final equilibrium temperature of two bodies of water with different initial temperatures. The problem involves a 5-gallon container of water at 212 degrees F mixed with 50 gallons of water at 50 degrees F, with a focus on the heat transfer between the two fluids.
Some participants have provided insights into potential errors in the initial setup of the heat transfer equation, suggesting that one side of the equation should account for heat loss. Others have expressed confusion regarding the calculations leading to an unexpected final temperature.
Participants are working under the constraints of the problem statement and are attempting to clarify the correct approach without reaching a definitive conclusion. There is an emphasis on ensuring the correct signs are used in the heat transfer equation.
If the final temperature is T degrees F, what are the values of Qlost and Qgained?trying_mybest said:Homework Statement:: A 5-gallon container of water (1 gal = 3.79 liter) at 212 degrees F is added to 50 gallons of water at 50 degrees F. What is the final equilibrium temperature in degrees C?
Relevant Equations:: Qlost = Qgained
Not really sure how to start this one.
And you'd like someone to guess where you are going wrong?trying_mybest said:I keep getting 0 for the final temp when it's supposed to be 18 C
Yes, but it will be simpler to do one conversion at the end than two at the start.trying_mybest said:Final temp should be ˚C.
That equation looks fine but what do you put for ##\Delta T_1## and ##\Delta T_2##?trying_mybest said:Final temp should be ˚C.
I used m1C∆T1 = m2C∆T2
I keep getting 0 for the final temp when it's supposed to be 18 C
Delta2 said:Well, i think the mistake lies right at the start.
$$m_1C(T_f-T_1)=m_2C(T_f-T_2)$$ is not correct, the correct is $$-m_1C(T_f-T_1)=m_2C(T_f-T_2)$$ because one body is losing heat (so the heat will be negative) and the other is gaining heat (so the heat will be positive).