Sodium oxide and water

Write equations for the reaction of (a) sodium oxide and water (b) sodium peroxide and water ... 

Sodium Oxide and Water. Support a porcelain crucible cover on a triangle and heat it to redness while it is thus hot, place upon it, by means of iron pincers, a piece of sodium the size of a small pea. Remove the burner and let the sodium bum. When cold dissolve the white oxide in a few cubic centimeters of water and test the solution with litmus. Notice some effervescence when the oxide is dissolving. Note that the solution turns litmus blue and feels very slippery when rubbed between the fingers. 

The word equation must show the reactants, sodium oxide and water, to the left of the arrow. The product, sodium hydroxide, must appear to the right of the arrow. 

No reaction takes place below 500°C when sodium cyanide and sodium hydroxide are heated in the absence of water and oxygen. Above 500°C, sodium carbonate, sodium cyanamide [19981-17-0] sodium oxide, and hydrogen are produced. In the presence of small amounts of water at 500°C decomposition occurs with the formation of ammonia and sodium formate, and the latter is converted into sodium carbonate and hydrogen by the caustic soda. In the presence of excess oxygen, sodium carbonate, nitrogen, and water are produced (53). 

Write a balanced chemical equation for (a) the reaction between sodium hydride and water (b) the formation of synthesis gas (c) the hydrogenation of ethene, H,C= GH2, and give the oxidation number of the carbon atoms in the reactant and product (d) the reaction of magnesium with hydrochloric acid. 

In the above process, finely divided iron oxide combined with sodium oxide and silica or alumina is used as the catalyst. The reaction is favored (as per Le Chatelier s principle) by high pressure and low temperature. However, a temperature of 500 to 550°C is employed to enhance the reaction rate and prevent catalyst deactivation. Although at 200°C and 250 atm the equihbrium may yield up to 90% ammonia, the product yield is too slow. The sources of hydrogen in commercial processes include natural gas, refinery gas, water gas, coal gas, water (electrolysis) and fuel oil, and the nitrogen source is liquefied air. 

Reactions (9a) and (9b) proceed concurrently nitrous oxide first reacts with molten sodium amide to form sodium azide and water vapour. The latter then reacts with another molecule of sodium azide, hydrolysing it with the formation of sodium hydroxide and ammonium (9b). 

The reaction between sodium metal and water is shown in the Sodium and Potassium in Water movie eChapter 14.14). Write and balance the equation for this reaction. Is this an oxidation-reduction reaction If so, identify the oxidizing and reducing agents. 

Attempts by A. W. Titherley to make sodium imide, Na2NH, by the action of ammonia on sodium oxide gave sodamide, NaNH2t and water Na20+2NH3 ->2NaNH2+H20. The water at once decomposes the sodamide, forming sodium hydroxide and ammonia, but if the action be suddenly stopped some of the primary product—sodamide—can be obtained sodium oxide and sodamide do not react to any appreciable extent. Bee potassium and sodium amides for the properties. 

Calcium oxide and water yield calcium hydroxide a composition reaction. Calcium chloride and sodium carbonate yield calcium carbonate and sodium chloride a double displacement reaction. 

Acetic anhydride is produced by the direct oxidation of ethylene in the presence of air. The synthesis of salicylic acid involves the combination of several reactants. Sodium hydroxide (NaOH) reacts with phenol (CeHsOH) to give sodium phenolate and water. Sodium phenolate reacts with carbon dioxide (CO2) to obtain sodium salicylate. The subsequent acidification with H2SO4 leads to pure salicylic acid and sodium sulfate. 

Ghloroheptinenearsinic acid.—The above oxide (JliJi parts) in 400 parts of acetone is treated with 8 per cent, hydrogen peroxide until oxidation is complete. The solution is shaken with 500 parts of ether and the ethereal layer washed with dilute sodium hydroxide and water. The aqueous alkaline solution is acidified with hydrochloric acid and concentrated in a vacuum at 60° to 70° C. until the arsinic acid crystallises. It forms shining white plates, M.pt. 115° C., soluble in water, giving a neutral solution. It yields a water-soluble sodium salt. 

The reaction proceeds in high yield as evidenced by the quantitative isolation of PhaBi from the reaction mixture, The reaction can be made catalytic by using iV-bromosuc-cinimide as the oxidant in the presence of sodium carbonate and water with acetonitrile as the solvent". PhaBiXa (where X = halide, acetate , etc.) can be used under basic conditions. Similar oxidations under aqueous conditions are effected with NaBiOa. ... 

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