The process for producing hydrogen gas according to the present invention consists of reacting aluminum with water in the presence of sodium hydroxide as a catalyst. How many moles of hydrogen can be produced from 8.40 grams of aluminum and excess sodium hydroxide? The reaction of aluminum and sodium hydroxide generates buckets of hydrogen. Al is amphoteric in nature, so it can react with both acid and base. An apparatus for carrying out the method is also described. The types of reactions found to occur between aluminum, sodium hydroxide, and water are shown below: The lacquer and labels on the cans are a bit of a nuisance, they block the lye from getting to the outside of the cans. Even using chunks of aluminum cut from an old window frame, the solution got so hot, it boiled. The reaction is highly exothermic. Stockburger et.al. observed, as well as the regeneration of sodium hydroxide via the precipitation of aluminum hydroxide. When aluminum and sodium hydroxide come into contact with one another, there is quite a vigorous reaction. Become … On treatment with NaOH, Al gives sodium aluminate salt and hydrogen gas. Hence, 0.466 moles of hydrogen gas are produced. The white powdery stuff is mostly aluminum oxide with a bit of sodium hydroxide. (11) described hydrogen generators in which aluminum was reacted with an aqueous solution of 5.75 M sodium hydroxide. The water has to be replenished often as it gets cracked away to oxidize the aluminum and release hydrogen. Not surprisingly, the preferred embodiment of the invention is the production of hydrogen from aluminium spheres and sodium hydroxide solution. 2NaOH + 2Al +2H2O = 2NaAlO2 + 3H2 Shredded cans might be better. We had to hold a long tube vertically over a jar to condense the steam and let it run back into the jar. Steam and let it run back into the jar acid and base from an window. 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