OBJECTIVE:
APPARATUS:
PRECAUTIONS:
You might expect to find Lv, of the nitrogen by setting
We can avoid this difficulty by noting that QAl is also the heat needed to warm the same aluminum cylinder to from Tb to Tr. You can measure this heat by placing the cold aluminum cylinder (at temperature Tb) in a ``calorimeter'' that contains water and observing the change in temperature of the water, - T, -provided that the final temperature of the water, Tf, is room temperature, Tr. It is hard to arrange for Tf to end up exactly at room temperature, but if Tf is close to Tr, one can accurately correct the calorimeter data for the small additional heat term, namely mAlcAl(Tr - Tf), since over the small Tr - Tf interval, cAl = 0.212 cal/g/K is constant.
SUGGESTIONS ON PROCEDURE:
How much of the N2 mass change was caused by the heat from the cylinder? If a-b and c-d were parallel, it would be the vertical distance between these lines. But c-d ordinarily has a smaller slope than a-b, possibly because the evaporation of liquid nitrogen between b and c has cooled the upper part of the flask.
Hence we use the average of the two rates of fall by drawing a vertical line through e, (the midpoint of line b-c). Then f-g estimates the mass, mN, evaporated by the heat from the cylinder.
Hence QAl will be the heat to warm the Al cylinder in the calorimeter to Tf plus the mass of the cylinder x (specific heat of aluminum) x (Tr - Tf).
Specifically if:
Lv = latent heat of vaporization of nitrogen
mN = mass of nitrogen evaporated by heat from the cylinder
mAl, cAl = mass and specific heat of Al cylinder
Ti = initial temperature of water and calorimeter
mw, cw = mass and specific heat of water
mc, cc = mass and specific heat of calorimeter and stirrer
ht = heat capacity of immersed part of thermometer,
then, if we neglect ht:
OPTIONAL: