Sure, approximately. In water the depression is 1.853 K·kg/mol. Multiply this by the moles of solutes in the beer per kg solvent. To do this you will have to work out the weights of alcohol and extract and water from the the Balling formula. Converting weight of alcohol to moles is trivial but for extract less so. What to use for the molecular weight? At least the molecular weight of triose. If we do that it gives a molecular weight almost 10 times that of ethanol. And we know the average molecular weight of extract is going to be more than that because of 4 unit and up sugars in it. An RDF of 50 - 60% is typical so that a beer with OE of 12 might exhibit an apparent extract of extract of 2 - 3 °P and have TE of 4.8 to 5 °P meaning a liter of it contains 48 to 50 grams of extract. Using 3*180 as the molecular weight of the extract we'd have 0.09 to 0.092 moles of extract. Such a beer would be about 6% ABV or about 4.7 ABW and thus contain about 47 grams of alcohol per liter which is 47/46 which is a tad over a mole. Thus it looks as if the alcohol will be the dominant factor. Our liter of beer is 6% alcohol and thus contains 940 cc of water with 47 grams of extract in it. We could work out the details and get the exact amount of water but for illustration lets wag it at 930 grams water. The depression is then
dT = 1.853*0.092/0.940 + 1.853*1/0.940 = 0.18 + 1.97 °C