Still wrong. You're oversimplifying, as discussed. This is not a first law of thermodynamics problem it is a: - convection heat loss problem (ice to whiskey) - conduction heat loss problem (ice to whiskey) - laminar flow problem (convection caused by thermoclines within whiskey) Do you understand the difference between "accuracy" and "precision?" You have some very precise calculations going on there - numbers and equations and logic oh my - but you do not have any accuracy as to what you're calculating. Yes, in a completely magical closed system something would have to lose so many joules in order to cool so many kelvin. And then the real world stepped in and smashed your dreams. You keep holding on to this as if wishing would make it true: It does. It really does. All the stuff you're discounting is the difference between "real world performance" and "ideal performance" and even "ideal performance" doesn't get anywhere without conduction and convection at a bare minimum. I know that you only want to use the math that you understand, but the math you don't understand is why I'm going to keep telling you you're wrong. And once more with feeling: I wouldn't model this. Period. I'd test it, fit a curve to it and use the data empirically in the future. When you model a complex system with a simplification bad things happen.That amount of energy is calculated with this formula:
Q = cp m dT
It doesn’t matter how you cool it, the answer is always the same.