<報文>酸化ゲルマニウムの水素による還元平衡について

概要

論文の詳細を見る
The equilibrium in the reduction of germanium dioxide by hydrogen was measured by the flow method. The reaction between GeO_2 and H_2 is shown as follows : 1/2 GeO_2(s)+H_2(g)=1/2Ge(s)+H_2O(g) The equilibrium constant and the standard free energy change of the reaction was determined from the experimental results within the range of temperature 410-500℃. The simple experimental equations representing the temperature dependence of the reaction are obtained as follow : 1/2 GeO_2(s)+H_2(g)=1/2 Ge(s)+H_2O(g), log K_p=-2,734/T+2.28 ΔF°=12,508-10.43T By combining the above equations with the preliminary data on the equilibrium reaction between H_2 and O_2,the thermodynamic equations are deduced for the illustration of the dissociation of germanium dioxide. GeO_2(s)=Ge(s)+1/2 O_2(g), ΔF°=141,156+6.82T logT-59.58T log PO_2=-30,854/T-1.49log T+13.02 From this result the heat of formation of germanium dioxide-141.8Kcal./mole at 298°K is obtained by permitting the use of known entropy data.
東北大学の論文
1956-02-20