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(1) From the experimental study of the nitrogenation of calcium carbide the author concluded its mechanism to be as follows: (a) adsorptions of nitrogen on the carbide, (b) formation of intermediate compound Ca(CN)2 temporarily, (c) breaking of Ca(CN)2 into CaCN2 and C. (2) Equations for this (gas-solid) reaction velocity were derived from above view. For constant temperature and pressure (Remark: Graphics omitted.) and for changing pressure (Remark: Graphics omitted.) (3) The coincidence of these equations with the experimental results were discussed. (4) The heat of activation for the reaction of the adsorbed nitrogen and carbide to form calcium cyanide was calculated to be approximately 86 Cal./mol.

(1) An interpretation on the real meaning of the observed oxidation velocity of ferrous hydroxide under the conditions of the author’s experiments was given to prevent misunderstanding of the author’s papers. (2) The reason, why the experimental conditions, under which the author’s measurements were carried out, were adopted, was described. (3) It was discussed that the oxidation velocity of ferrous hydroxide, observed by A. Krause under quite different conditions, will have quite a different meaning as that, observed by the author. The difference of the real meaning of the observed reaction velocity, caused by the difference of the experimental conditions, will explain why the effect of temperature, which was negligible under the author’s conditions, was found by A. Krause to be very great.

Estimation of the volume of hydrogen consumed by a static method with Cu-Cr-O under atmospheric pressure of hydrogen at 180°C by hydrogenation of whale oil was-studied kinetically. It was observed that the reaction is zero order to the concentration of the molecule to be hydrogenized, and, in spite of it, the reaction velocity gradually decreases due to the reversible poisoning of catalyst. An assumption was made that a poisonous substance is formed in the process of catalysis, and that its amount is proportional to the degree of hydrogenation. The following formula is presented. dx/dt=K_1(N_o-K_2x)

It has been experimentally determined that the velocity of reaction between nitrogen and calcium carbide at high temperatures is not directly proportional to the nitrogen-pressure, but there exists the following relation: (Remark: Graphics omitted.) \oindentwhere P denotes the pressure, K and α certain constants depending upon temperature and other conditions of the reaction.It has also been found that the higher the temperature the greater is the effect of pressure-increase to the velocity of reaction, though the effect of the pressure-increase becomes smaller at higher pressures. At lower pressures the velocity of the reaction is nearly proportional to the pressure.

1. Assumed as monomolecular reaction, the velocity of the decom-position of potassium monochloracetate in aqueous solutions is measured, K_25°=0.837×10^-6 and K_30°=3.21×10^-62. The velocities of the following reactions are measured, CH2CLCOOK+KOH = CH2OHCOOK+KCL K_20°=0.227×10^-4, K_25°=0.521×10^-4 and K_30°=1.23×10^-4 CH2CLCOONa+NaOH=CH2OHCOONa+NaCl K_25°=0.381×10^-4, K_30°=0.704×10^-4 and K_35°=2.18×10^-4The velocity constant of potassium salt is larger than that of sodium salt. 3. The reaction velocity of potassium monochloracetate with potassium hydroxide is retarded by the presence of another salt (i.e. KNO3).

(1) A method for calculating both reaction velocity and activation energy in the case when the reaction has been carried out in the thermal separation column of Clusius and Dickel has been described. (2) The method has been applied to the polymerisation reaction of acetylene previously investigated by the present authors. (3) It has been found that the calculated heat of activation is slightly smaller than our preliminary value, but larger than the directly observed value by Taylor and van Hook, and that the calculated velocity constants are several times larger than those hitherto have been observed.

1. The photochemical reversible reaction of the alkaline solution of malachite green was studied with the quartz-mercury-lamp, and its nature was discussed. 2. The reaction velocities were determined both in the light and the dark reaction, using Nutting’s spectro-photometer. The former is proportional to the intensity of light and the latter to the concentration of the alkali added. 3. The temperature coefficient of the reaction velocity of the light reaction was found to be unity at the interval between 25° and 35°C. 4. Equation of the reaction of first order was derived with approximation for the light reaction.

1. The oxidation velocity of stannous hydroxide suspended in sodium carbonate solution of various concentrations by means of air was studied. The oxidation velocity was independent of the quantity of stannous hydroxide. 2. The effect of the concentration of sodium carbonate on the reaction velocity was small. 3. It was ascertained that sodium stannite is oxidized rapidly, while stannous hydroxide is oxidized very slowly by means of air. 4. The effect of temperature on the reaction was small.

(1) The oxidation velocity of sodium sulphite solution was observed when air is passed at various velocities. (2) It was found that the oxidation velocities are independent of the concentration of sodium sulphite and the velocity constant was expressed as a linear function of the velocity of air passed. (3) The dissolution velocity of oxygen into water when the concentration of oxygen in the surface layer is kept zero, was calculated from the obserbed reaction velocity, and it was found to be expressed as a linear function of the velocity of air passed. (4) An interpretation of the mechanism of this reaction under the observed conditions was given. (5) The maximum value of the ratio of the total number of molecules of oxygen which enter into water to the total number of molecules of oxygen which collide with the unit boundary surface per unit of time at 25°C. was calculated from the observed results.