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Old Feb 11th 2019, 05:19 PM   #1
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Thermal Equilibrium Question

2kg of ice is at -10C is mixed with 15kg of water at 25C.
What is the final temp when equilibrium is achieved.

Q = Energy
M = mass
c = Heat capacity
∆T = Change in temperature
W = Water
I = Ice

Heat capacity for water is 4200 J/Kg
Heat capacity for Ice is 2100 J/Kg

Well, i approached this question by first finding: Q Of water (lost) = Q Of Ice (Gained)
Q=M(w) x C(w) x ∆T(w) --> 15 x 4200 x (25 - T) ...
= 63000(25-T)
[T here is temperature equilibrium]

Ice would be 2 x 2100 x{i don't know what to insert here}

Note: I think the ice is also melting and requires some latent heat of fusion.
Which was [Fusion heat] = 3.34 x 10^5 J/Kg.

I'm just lost at this point from the ice ∆T.
Any suggestions what to do at that stage?

Last edited by IshaanM8; Feb 11th 2019 at 05:20 PM. Reason: Comma errors
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Old Feb 13th 2019, 10:27 AM   #2
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Join Date: Jun 2010
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Posts: 419
Hi,

This is a clasic problem. The usual approach is to
taking the two masses together as an abiabatic system, the event
is called "thermal equilibration."

Here is an example:

Citris Concentrate
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