{"id":120,"date":"2016-09-07T15:14:12","date_gmt":"2016-09-07T15:14:12","guid":{"rendered":"http:\/\/www.experimentoscientificos.es\/?p=120"},"modified":"2022-04-27T13:43:39","modified_gmt":"2022-04-27T13:43:39","slug":"producir-hidrogeno","status":"publish","type":"post","link":"https:\/\/www.experimentoscientificos.es\/en\/producir-hidrogeno\/","title":{"rendered":"Producing Hydrogen, H2, with Aluminium and HCl"},"content":{"rendered":"
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EXPERIMENT SHEET TO PRODUCE HYDROGEN<\/h2>\n\n\n\n\n\n\n
Theme<\/strong><\/td>\nRedox Reaction<\/a><\/td>\n<\/tr>\n
Category<\/strong><\/td>\nChemistry Experiments<\/a><\/td>\n<\/tr>\n
Main product<\/strong><\/td>\nHydrochloric Acid<\/td>\n<\/tr>\n
Short description<\/strong><\/td>\nIn this experiment we are going to look at the oxidation reaction between the Aluminium and Hydrochloric Acid<\/strong>. In this reaction, it will to produce hydrogen gas, H2<\/strong>. Hydrogen gas is a gas that weighs less than air (if you inflate a hydrogen balloon, it will fly like a helium balloon does). Hydrogen is not only light, it is also a flammable gas, so you have to be very careful, a spark or heat could cause it to explode.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

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REACTION BETWEEN ALUMINIUM AND HYDROCHLORIC ACID<\/h2>\n

The basic reaction that takes place is as follows:<\/p>\n

6 HCl + 2Al -> 2AlCl3<\/sub> + 3H2<\/sub><\/strong><\/p>\n

The reaction between aluminium and hydrochloric acid is an oxidation-reduction reaction, resulting in aluminium chloride and hydrogen gas. In all oxidation-reduction reaction<\/a>which is produced by the difference in oxidation potential<\/a> of the elements, there is one component that loses electrons (by oxidising) and another that gains electrons (by reducing). In this reaction, Aluminium is oxidised (loses electrons), going from Aluminium metal, with oxidation state 0, to Aluminium 3+ ion and Hydrogen is reduced (gains electrons), going from proton H+ to hydrogen gas. The oxidation potentials of each of the elements can be seen here:<\/p>\n

2H+(aq) + 2e- \u2192 H2(g) 0V<\/p>\n

Al(s) \u2192 Al3+(aq) + 3e- 1.676V<\/p>\n

The oxidation-reduction reaction between aluminium and hydrochloric acid is a strongly exothermic reaction, which occurs spontaneously (without the need for activation energy). In this case it is the hydrogen ion that acts as an oxidant for the metal, reducing it to hydrogen gas H2<\/sub>which is highly flammable, so the experiment has to be carried out very carefully.<\/p>\n

EXPERIMENT TO PRODUCE HYDROGEN WITH HYDROCHLORIC ACID AND ALUMINIUM<\/h2>\n