The Pol
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It does. Just make sure you keep the crap out of it.
How do most do this? I already use SS mesh pads.
It does. Just make sure you keep the crap out of it.
Well, here is the "idea"...
Utilize (2) march pumps
(1) Therminator
(1) 10 gallons of ICE water
During the boil I clean my MLT.
Refill MLT with water and (3) gallons of ICE
After boil is complete operate ONE pump to recirc boiling wort through THERMINATOR back to the kettle to help sanitize therminator.
To chill, run both pumps at full flow. One to recirc ice water from MLT to the chiller and back to the MLT. The other pump will recirc the wort through the Therminator to the kettle through a QD fitting on the side of the kettle that is attached to a length of LocLine on the INside of the BK.
The PID thermocouple in the BK would monitor temp.
Would this work? I am looking to spend some money is all, is this an effective way to spend money?
I still dont get it...
If it will cool 10 gallons from boiling to 68F with 58F water in 5 minutes...
I am cooling 5 gallons from boiling to 68F with what starts as 32F with 20 pounds of ice augmenting the cooling. You are telling me that in 5 minutes I will have NO ice and my water will exceed 58F?
I wish there were a way to calcualte this accurately before I spend $400 to do it
Frankly, the advantage of plates/CFC external exchangers is the ability to just push the wort into your fermenter in one quick pass so I don't really see the advantage of a recirculate. You might say it's to chill the whole wort down quickly, but with icewater as the coolant, you can run the March full bore and drain 5 gallons within 5 minutes.
I must say, for $400, you could spend an extra $50 and install a hose bib in your garage, then you could use that and drain into your garage drain.
I still think the contained system is sexy. That was my initial plan to until I was shot down by naysayers... perhaps my pipedream lives???
That's about what I use, too, and I first use tap water to chill the wort before it exchanges heat with the ice water.Hmmm.... interesting Lonnie. So you need to use 4-5 seven pound bags of ice (i.e., 28-35 pounds) to bring 10g from 100 to pitching? That is way more than I would have guessed. Weird.
Yes, the HEX exhaust will melt that ice fast. Once it's gone, the entire cooling tank will heat up. I don't know how much "extra" cooling capacity the ice holds, but remember, it won't be 20 lbs after it chills 5 gals down to 32º - maybe only 1/3 or 1/2 of that.I am cooling 5 gallons from boiling to 68F with what starts as 32F with 20 pounds of ice augmenting the cooling. You are telling me that in 5 minutes I will have NO ice and my water will exceed 58F?
No drain in garage...
Prefer it to be self contained
Q=mc(T2-T1)
1572787 cal x (1 Joule / .2390 cal) = 6580699 J
6580699J = 35789g x 4.1813J/(g·K) x [ 66 - T1 ]
44 = 66 - T1
T1 = 22C = 72F
That is assuming 100% efficiency, but I think this idea has merit.
Here's a similar "problem" I found and how it's worked out:
5. The temperature in the freezer compartment of a typical household refrigerator is about
– 15oC. Thus, an ice cube taken from the freezer must first warm up to 0oC before it will begin to melt. The specific heat of ice is 0.51 cal/g-oC and its latent heat of fusion is 80 cal/g.
Imagine that a 10 g cube of ice at –15oC is taken from the freezer and added to 100 g of water in a Styrofoam cup. The temperature of the 100 g of water is initially 22oC. What is the final temperature of the water after all the ice has melted? Show all your work.
a. Begin by determining the amount of energy required to heat the ice cube from –15oC to 0oC. Assume that none of the ice melts.
The heat to warm the ice to 0C is:
Heat = 10 grams X 15 C X 0.51 cal/gC = 76.5 cal
b. Next, find the amount of energy required to melt the ice cube. Show your work.
10 grams X 80 cal/g= 800 cal
c. The sum of your answers to parts a and b represents the total amount of heat required to warm the ice cube up to 0oC and melt it. Since the ice cube was added to a cup of water, this energy will come from the water, causing its temperature to decrease. Calculate the temperature of the cup of water after the ice cube has melted.
876.5 cal = 100 grams of water X T X 1 cal/gC
T= 8.8C
The water started at 22C, so the final temperature would be 22C-8.8C= 13.2C
d. Your answer to part c is not the final temperature of the mixture, because after the ice cube has melted it is still at 0oC. Thus the cup now contains 10 g of water at 0oC and 100 g of water at the temperature found in part c. These two samples of water will exchange heat until they reach an equilibrium condition. Set up a table like the one we used last quarter to work out the final temperature. To make the calculations easier, determine the amount of heat necessary to lower the temperature of the 100g of water by 0.2oC. Then determine the temperature of the 10 g of cold water when it receives this heat. Continue until you have determined the equilibrium temperature.\
For your example it wouldn't be 10 grams of ice, it would be 15,000 grams. Your wort would be about 19,000 grams at 100c and your coolant water is 19,000 grams at (tap temp). Since the wort and water are both liquid, you might just say that your "liquid" is 38,000 grams at (the average between your 100c wort and tap temp water).
Here's a similar "problem" I found and how it's worked out:
5. The temperature in the freezer compartment of a typical household refrigerator is about
15oC. Thus, an ice cube taken from the freezer must first warm up to 0oC before it will begin to melt. The specific heat of ice is 0.51 cal/g-oC and its latent heat of fusion is 80 cal/g.
Imagine that a 10 g cube of ice at 15oC is taken from the freezer and added to 100 g of water in a Styrofoam cup. The temperature of the 100 g of water is initially 22oC. What is the final temperature of the water after all the ice has melted? Show all your work.
a. Begin by determining the amount of energy required to heat the ice cube from 15oC to 0oC. Assume that none of the ice melts.
The heat to warm the ice to 0C is:
Heat = 10 grams X 15 C X 0.51 cal/gC = 76.5 cal
b. Next, find the amount of energy required to melt the ice cube. Show your work.
10 grams X 80 cal/g= 800 cal
c. The sum of your answers to parts a and b represents the total amount of heat required to warm the ice cube up to 0oC and melt it. Since the ice cube was added to a cup of water, this energy will come from the water, causing its temperature to decrease. Calculate the temperature of the cup of water after the ice cube has melted.
876.5 cal = 100 grams of water X T X 1 cal/gC
T= 8.8C
The water started at 22C, so the final temperature would be 22C-8.8C= 13.2C
d. Your answer to part c is not the final temperature of the mixture, because after the ice cube has melted it is still at 0oC. Thus the cup now contains 10 g of water at 0oC and 100 g of water at the temperature found in part c. These two samples of water will exchange heat until they reach an equilibrium condition. Set up a table like the one we used last quarter to work out the final temperature. To make the calculations easier, determine the amount of heat necessary to lower the temperature of the 100g of water by 0.2oC. Then determine the temperature of the 10 g of cold water when it receives this heat. Continue until you have determined the equilibrium temperature.\
For your example it wouldn't be 10 grams of ice, it would be 15,000 grams. Your wort would be about 19,000 grams at 100c and your coolant water is 19,000 grams at (tap temp). Since the wort and water are both liquid, you might just say that your "liquid" is 38,000 grams at (the average between your 100c wort and tap temp water).
So basically, you need twice as much ice to chill your wort to avoid using tap water from a hose... and all of this from one of the forum's big proponent of no-chill brewing?
So basically, you need twice as much ice to chill your wort to avoid using tap water from a hose... and all of this from one of the forum's big proponent of no-chill brewing?
So basically, you need twice as much ice to chill your wort to avoid using tap water from a hose... and all of this from one of the forum's big proponent of no-chill brewing?
Sparks, I may have missed something in all of those calculations. But, at 7-10 GPM, a hose uses at least 100 gallons, more likely double.
Pol, I was referring to the amount of water needed from a tap using no recirculation. Guess I didn't make that very clear.
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