[satterly-patterson] latent HEATS 127 



rod at 17°C. was lowered into the liquid 270 cc. of gas was evolved. 

 The density of ethane gas at the time of the experiment was '00126 

 gm. per cc. 



8-9X087X107 



Hence L = 



270X -00126 

 = 244 calories per gm. 



As a check the experiment was repeated with a narrow calori- 

 meter weighing 74-4 gm. The room temperature was 17°C. This 

 calorimeter was attached to a string as before and lowered into the 

 liquid ethane (at — 90°C.) contained in the thermos bottle, 1920 cc. 

 of ethane being evolved. The calorimeter was then quickly withdrawn, 

 emptied of ethane and 40 cc. of water at 18-5°C. was poured in. 

 The final temperature of the water was 4°C. Hence we have the 

 following equations: 



74-4XsX(17+9Q) = 1920X-00126XL 

 74-4XSX (4+90) =40X IX (18-5-4-0) 

 where s = average specific heat of the metal from room temperatures 

 down to -90°C. 



Combining these, we get 



107X40X14-5 



L = 



94 X 1920 X -00126 

 = 273 calories per gm. 



Hence the mean value for the latent heat of ethane is about 260 

 calories per gm. 



The above results do not pretend to be within less than 5% of 

 the correct values, but, such as they are, they have proved useful in 

 designing machinery for future liquefaction purposes. 



Universitv of Toronto. 



