BETWEEN THE CONDITIONS OF A CHEMICAL CHANGE AND ITS AMOUNT. 127 
Table IV. 
Volume, 993 cub. centims. 
Temperature, 30°. 
Hydric sulphate, 746. 
Hydric iodide, 1 950. 
Sodic peroxide, 74. 
Sodic hyposulphite (one measure), 13-3. 
Volume, 694 cub. centims. 
Temperature, 17°. 
Hydro-sodic carbonate, 4760. 
Potassic iodide, 5180. 
Sodic peroxide, 35-7. 
Sodic hyposulphite (one measure), 10-7. 
Volume, 993 cub. centims. 
Temperature, 0°. 
Hydric sulphate, 18700. 
Potassic iodide, 1208. 
Sodic peroxide, 59-5. 
Sodic hyposulphite (one measure), 10-9. 
Intervals, t'—t. 
Intervals, t’—t. 
Intervals, t'—t. 
Observed. 
Calculated, 
*.=•0242. 
Observed. 
Calculated, 
*=•085. 
Observed. 
Calculated, 
*=•0043. 
2*4.2 
2-40 
1*17 
1*17 
14-27 
13-8 
2-50 
2-55 
1-30 
1-30 
14-77 
14-6 
2-71 
2-72 
1-45 
1-46 
31-38* 
32-4 
2*94 
2-91 
1-65 
1-66 
17-87 
18-1 
3-10 
3-13 
1-93 
1-93 
19-62 
19-6 
3-40 
3-39 
2-33 
2-32 
21-45 
21-4 
3-68 
3-69 
2-88 
2-89 
2365 
23-6 
4-07 
4-05 
3-78 
3-83 
26-37 
26*3 
4-52 
4-49 
5-70 
5-71 
5*02 
5-04 
11-73 
11-54 
5-77 
5-74 
6*71 
6-67 
7-92 
7-97 
9-77 
9-88 
12-91 
13-00 
19-00 
19-00 
37-00 
36-70 
Volume, 993 cub. centims. 
Volume, 993 cub. centims. 
Volume, 993 cub. centims. 
Temperature, 30’. 
Temperature, 30°. 
Temperature, 50°. 
Hydric sulphate, 112000. 
Hydric chloride, 13900. 
Hydric sulphate, 18700. 
Potassic iodide, 604. 
Potassic iodide, 604. 
Potassic iodide, 1208. 
Sodic peroxide, 34-9. 
Sodic peroxide, 27'5. 
Sodic peroxide, 37"8. 
Sodic hyposulphite (one measure), 21-9. 
Sodic hyposulphite (one measure), 14-1. 
Sodic hyposulphite (one measure), 13-4. 
Intervals, t’—t. 
Intervals, f—t. 
Interva 
Is, t'-t. 
Observed. 
Calculated, 
Observed. 
Calculated, 
Observed. 
Calculated, 
*=•0949. 
* = •0268. 
*=•131. 
2-31 
2-32 
6-53 
6-56 
1-00 
1*01 
2-98 
2-98 
8-05 
7-96 
1-18 
1-17 
4-15 
4-17 
10-13 
10-13 
1-37 
1-38 
7-01 
7-00 
13-95 
14-00 
1-70 
1-70 
30-38 
.30-27 
22;42 
22-60 
2-20 
2-19 
67*08 
66-84 
3-08 
3-09 
- 
5-33 
5-32 
The discrepancy between the observed and calculated intervals in the earlier experiments 
of the set made at 0° C. depends upon the difficulty which was experienced in managing 
the temperature. If it rose at all the rate of change was of course increased, and if it 
fell it was increased also by the separation of some of the water from the acid solution 
in the form of ice. With this exception it will be seen that the calculated and observed 
intervals agree 'very closely. Hence we conclude that whether the solution contains in 
each cub. centim. 746 millionths of a gramme of hydric sulphate, or 150 times that 
* Double interval. 
s 2 
