Iron chloride, reaction with water

Interaction of the 3 2 complex with iron(III) chloride and calcium oxide, mercury oxide or silver oxide was usually too violent for preparative purposes, but zinc oxide was satisfactory. Reaction with water was violent. 

CHEMICAL PROPERTIES highly reactive hazardous polymerization may occur reacts with acids, alkalies, strong oxidizers, chlorides of iron, oxides of iron and aluminum, aluminum and tin may also undergo runaway reaction with water FP (-20°C, -4°F) LFLAJFL (3%, 100%) AT (429°C, 804°F) HF (-52.6 kJ/mol gas at 25°C). 

Write balanced chemical equations for each of the following verbal descriptions (a) Vanadium oxytrichloride (VOCI3) is formed by the reaction of vanadium(lll) chloride with oxygen, (b) Niobium(V) oxide is reduced to the metal with hydrogen gas. (c) Iron(lll) ion in aqueous solution is reduced to iron(ll) ion in the presence of zinc dust, (d) Niobium(V) chloride reacts with water to yield crystals of niobic acid (HNb03). 

Methylene chloride is one of the more stable of the chlorinated hydrocarbon solvents. Its initial thermal degradation temperature is 120°C in dry air (1). This temperature decreases as the moisture content increases. The reaction produces mainly HCl with trace amounts of phosgene. Decomposition under these conditions can be inhibited by the addition of small quantities (0.0001—1.0%) of phenoHc compounds, eg, phenol, hydroquinone, -cresol, resorcinol, thymol, and 1-naphthol (2). Stabilization may also be effected by the addition of small amounts of amines (3) or a mixture of nitromethane and 1,4-dioxane. The latter diminishes attack on aluminum and inhibits kon-catalyzed reactions of methylene chloride (4). The addition of small amounts of epoxides can also inhibit aluminum reactions catalyzed by iron (5). On prolonged contact with water, methylene chloride hydrolyzes very slowly, forming HCl as the primary product. On prolonged heating with water in a sealed vessel at 140—170°C, methylene chloride yields formaldehyde and hydrochloric acid as shown by the following equation (6). 

The corrosivity of a salt solution depends upon the nature of the ions present in the solution. Those salts which give an alkaline reaction will retard the corrosion of the iron as compared with the action of pure water, and those which give a neutral reaction will not normally accelerate the corrosion rate appreciably except in so far as the increased conductivity of the solution in comparison with water permits galvanic effects to assume greater importance. Chlorides are dangerous because of the ability of the anions to penetrate otherwise impervious barriers of corrosion products. 

The reaction was applied with success to unprotected reducing disaccharides [92,93]. The use of iron(III) chloride in ethanol-water gave similar results [94] (see footnote 1). 

Pour a little water into the retort with the residual iron chloride and immerse litmus paper into the solution. Explain what happens. Write the equation of the reaction. 

---