Thermodynamic Entropy Clarification

[bpaterni]

Homework Statement

We mix 0.6 kg of water at a temperature of 25°C with 0.8 kg of alcohol at 30.5°C. They
come to equilibrium. (Here's some useful data: The specific heat capacity for water is 1
kcal/kg°C = 4186 J/kg°C, and for alcohol it is 0.58 kcal/kg°C = 2430 J/kg°C

What is the change in entropy (in J/K) of the system when the two are mixed?

Homework Equations

∆S = ∆Sw + ∆Sa = Mw*Cw*ln(Tf /TW) + Ma*Ca*ln(Tf /Ta)

The Attempt at a Solution

I've calculated the final temperature to be 300.55 K or 27.4 C

so now the equation looks like:
.6*4186*Ln(Tf/Tw) + .6*2430*Ln(Tf/Ta) = dS

The problem is, do I use Kelvin or Celsius for the entropy calculation? I get two totally different values if I do either one... .0794 with K or 21.87 with C.

 

[rl.bhat]

You have to use Kelvin.