The tablets consisting of chemically purest Mg(OH)
2 and 0-1.5wt. per cent Fe
2O
3 were fired at 1000°-1550°C to examine the appearance after the firing as well as the microstructure.
The firing shrinkage and the bulk density began to increase markedly from 1000° to 1200°C (Figs. 1-4). At 1200°C the coloured regions, which had developed by the diffusion of iron from Fe
2O
3 grains, began to spread abruptly with the remarkable growth of periclase crystals. From the results mentioned above, it may be inferred that the sintering of Mg(OH)
2 occurs in two successive stages; (1) up to 1200°C the periclase crystals formed by the decomposition of Mg(OH)
2 come into intimate contact each other showing the remarkable shrinkage of the specimens, and (2) in the second stage during which the growth of periclase crystals takes place with the rapid diffusion of iron from Fe
2O
3 through the contact points between periclase grains.
The mechanism of the reaction of Fe
2O
3 and MgO examined by poralization microscope and X-ray diffraction may be interpreted clearly with the aid of the phase diagram of the binary system MgO and Fe
2O
3 (B. Phillips, S. Somiya, and A. Muan,
J. Am. Ceram. Soc., 44, 169 (1961)).
The reaction is a kind of the counter diffusion processes. MgO diffuses into Fe
2O
3 grains to form magnesioferrite. With the elevation of temperature, Fe
3O
4 content of the magnesioferrite becomes higher until it changes to very dark colour. On the other hand, Fe
2O
3 is reduced into ferrous state which duffuses into MgO to form a solid solution, magnesiowüstite. With increasing temperature the content of ferrous iron increases up to the saturation limit with a result that the further introduction of iron oxide to the periclase phase gives rise to the formation of magnesioferrite.
The acicular hematite crystals are exsoluted from the magnesioferrite during cooling, which distribute between the grains of magnesioferrite, as the solid solution limit of Fe
3O
4 decreases with decreasing temperature. Also magnesioferrite is exsoluted from magnesiowüstite and spread throughout the periclase phase, as the solid solution limit of FeO in periclase decreases grately with decreasing temperature.
The results of the experiments mentioned above suggest that the following conditions should be held in order to maintain the higher FeO content of magnesia clinker: (1) In order to enlarge the area of the solid solution limits of FeO in periclase, and of Fe
3O
4 in magnesioferrite, it is desirable that the firing temperature is kept as high as possible. (2) To maintain the conditions in higher temperature the clinkers should be cooled quickly. (3) To accelerate the reactions between Fe
2O
3 and MgO the grain size should be reduced as far as possible. In practice the refractories can not be cooled rapid enough to prevent the exsolution of FeO. If we consider only this phenomenon, it seems to be inferred that the magnesia clinker mineralized with Fe
2O
3 is not suitable for the fired refractories, and if the clinker mineralized with Fe
2O
3 is used, unburned refractories seem to be prefered rather than the fired ones.
From the experimental results concerning the relation between the firing shrinkage and Fe
2O
3 contents, it is suggested that only a small amount of Fe
2O
3 would be sufficient for the mineralizer of magnesia clinker.
During the heating up the growth of periclase grains proceeds gradually together with the diffusion of iron from Fe
2O
3 grains. Pores between the periclase grains, and perhaps the oxygen releases by the reduction of
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