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Aluminum Hydrochloric Acid Reaction

 We must have seen electric wires in between utility poles on road sides, silver utensils and coloured aluminium sheet for making roof. What the common thing in all of these is? 
They all are solid in form and metal. What do you think about diamond and sulphur powder? 
Both are nonmetals and can easily identify from metals. 
Metals have luster surface which can observe on copper and aluminum utensils. They are hard, malleable, ductile and good conductors of heat and electricity. 
The metallic lustre is caused by free electrons as they can reflect light.   
That is the reason; they are used as electric wires. 
The free electrons in metallic lattice are responsible for conductivity of metals.  
Due to metallic bond between free electrons and metal cation, metals show malleability and ductility. 
The disadvantage of these free electrons is corrosive nature if metal, which is due to oxygen gas in the atmosphere, creates an imbalance of electrons and positive ions in the metal and rust is produced. 
But we cannot draw wires of phosphorus and sulphur as they are non-metals and cannot drawn as wires. 
They are brittle and easily break also. 
Non-metals have less density and low melting and boiling points. On the contrary; metals are heavy with high density and high melting and boiling points. In periodic table out of all elements more than 75% elements are metal in nature and positioned at left side of table. 
All metal show electropositive nature as they can loss their valence shell electron to become stable. 
Therefore when a metal atom loses electrons it becomes metal cation. 

Let’s discuss some of the chemical properties of metals with different reagents. Metals can react with atmospheric oxygen and form metallic oxides. As the reactivity of metal increases, they can easily convert into metallic oxides. 
For example; sodium is highly reactive and quickly reacts with atmospheric air to form sodium oxide. 
Metallic oxides are alkaline in nature and forms ions in their aqueous solution such as sodium oxide reacts with water to form sodium hydroxide. Reaction of metal with acid depends on reactivity of metal atoms.  
Highly reactive metal can reacts with dilute acids with release of hydrogen gas while a less reactive metal reacts with strong acid under drastic conditions only. We can check the reactivity of metals in the reactivity series of them. 

According to this series; Lithium metal is most reactive and place at the top of series while noble metals such as Gold, Platinum are least reactive and place at the bottom of series. 
The reaction of metals with inorganic acids such as hydrochloric acids results the formation of metallic halide and hydrogen gas. 
The reaction of sodium with HCl forms sodium chloride and hydrogen gas. The reaction can be written as given below;

2Na + 2HCl  2NaCl + H2

But Copper and Silver cannot react with dilute HCl due to less reactivity. 
Aluminium metal can easily dissolve in dilute sulphuric acid or dilute hydrochloric acid. It forms soluble aluminium sulphate and release H2 gas with H2SO4 acid. 
Similarly with HCl, it forms AlCl3 (aluminium chloride) and H2 gas. 
Both reactions can be written as given below;
  • 2Al(s) + 3H2SO4(aq) → 2Al3+(aq) + 2SO42-(aq) + 3H2(g)

  • 2Al(s) + 6HCl(aq) → 2Al3+(aq) + 6Cl-(aq) + 3H2(g)
       
The reaction occurs violently and hydrogen gas comes out with whisper sound with the liberation of some heat.        

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From Yahoo Answers

Question:When aluminum foil is placed in hydrochloric acid, nothing happens for about 30 seconds or so. This is followed by vigorous bubbling and the eventual disappearance of the foil. Explain these observations.

Answers:The reaction that occurs is 2 Al + 6 HCL ---> 2 AlCl3 + 3 H2 So the bubbling gas is hydrogen. The reason there is a slight delay is that aluminum forms a very thin oxide layer which must be dissolved first.

Question:What is the mass of hydrogen gas released from 2.70g of aluminum metal and hydrochloric acid? (Balance the reaction first) __Al(s) + __HCl(aq) -->__AlCl3(aq) + __H2(g)

Answers:2 Al + 6 HCl = 2 AlCl3 + 3 H2 moles Al = 2.70 g/ 27 g/mol= 0.10 moles H2 = 0.10 x 3 / 2 =0.15 mass H2 = 0.15 mol x 2 g/mol= 0.30 g

Question:so i did a lab on this and i put metals such as lead, aluminum and manganese into both hydrochloric acid and sulfuric acid, but only magnesium and manganese had some reactions with both acids, im pretty sure my results are not right ....so how do i know whether a reaction took place or not? and if a reaction took place, is hydrogen gas produced in all cases?

Answers:Do you mean manganese or magnesium or both? Manganese is not a common school lab reagent. Magnesium expect vigorous reaction with dilute HCl and H2SO4 Manganese not a very fast reaction at all. Lead hardly any reaction seen Aluminium no (or slight) reaction due to impervious oxide coating (btw Aluminium is spelled that way in UK and other English speaking countries) In all cases hydrogen gas is released in case of magnesium heat evolved is appreciable.

Question:Which of the following compounds results from treating aluminum oxide with excess aqueous sulfuric acid and what are the steps to getting it? (b) [Al(H2O)6]2(SO4)3 (c) H[Al(OH)4] (d) Al2S3 (e) Al(OH)3

Answers:Al2O3 + 3H2SO4 -------- Al2(SO4)3 + 3 H2O The compound forms a hexahydrate in aqueous systems ( aqueous H2SO4 ). b is the answer this is a typical neutralization of a basic oxide withan acid forming a salt plus water.

From Youtube

Chemical Reactions: Hydrochloric Acid + Aluminium Foil Bomb :This was part 2 in a series of teaching resource videos designed to demonstrate what chemical reactions are. In reality, this was just a fun excuse to blow stuff up in the name of science. It shows that when you react an acid with a metal (in this case, HCl and aluminum foil) you get hydrogen gas plus a salt, in this case, aluminum chloride.

Metals vs Hydrochloric acid :WARNING: Wear gloves when using hydrochloric acid. This is very dangerous, strong and corrosive acid. In this video, I will show you the reactions of hydrochloric acid and metals. A lot of hydrogen gas is produced so be careful. YOU WILL NEED: - hydrochloric acid (I m using 33% concentraton) - a 100ml container - a gloves - zinc metal - copper metal - aluminum foil - an iron nail Let s get started. First is the zinc metal. You can see, very reactive in hydrochloric acid. Next, the copper. It doesn t seems it s reacting, but when you have copper oxide, hydrochloric acid dissolves the copper oxides and solution turns blue. But nothing else happens. Now the aluminum foil. Very reactive, but firstly, as you can see, it s very slow due the protective layer on the alimunum foil. When the layer is dissolved, aluminum starts reacting. The last is an iron nail. At the beggining you can see some bubbles of H2, but that is all. Thank you for whatching ! The next video is coming soon ! Please subscribe, rate and comment. FOLLOW AND TWEET ME ON TWITTER: twitter.com ASK ME A QUESTIONS HERE: ChemExperimentalist@gmail.com