It could stop because there wasn't enough magnesium or hydrochloric acid for the reaction to go to completion.
Hydrochloric acid
the chemicals in the magnesium dissolved in the viniger
the limiting factor varies between the magnesium and hydrochloric acid as there needs to be enough hydrogen for every magnesium..
Yes, when magnesium reacts with hydrochloric acid it is a single replacement reaction. The same is true for nearly all cases of a reaction between an acid and a metal.
No, it is a single displacement reaction. It can also be called a redox reaction. It is not an acid base reaction because although hydrochloric acid is obviously and acid, magnesium is a metal, not a base.
Magnesium Chloride.
magnesium chloride + hydrogen
the limiting factor varies between the magnesium and hydrochloric acid as there needs to be enough hydrogen for every magnesium..
Yes, when magnesium reacts with hydrochloric acid it is a single replacement reaction. The same is true for nearly all cases of a reaction between an acid and a metal.
No, it is a single displacement reaction. It can also be called a redox reaction. It is not an acid base reaction because although hydrochloric acid is obviously and acid, magnesium is a metal, not a base.
magnesium chloride + hydrogen
Magnesium Chloride.
This reaction is exothermic.
That a reaction has occurred between the magnesium & hydrochloric acid: Mg(s) + HCL(aq) --> MgCl(aq) + H2(g)
Magnesium hydroxide plus hydrochloric acid yields magnesium chloride plus water. Mg(OH)2 + 2HCl = MgCl2 + 2H2O
The reaction is: Mg + 2HCL = MgCl2 + H2
The equation for the reaction between magnesium and hydrochloric acid is Mg + 2HCl --> MgCl2 + H2
Concentrated hydrochloric acid is more reactive than dilute hydrochloric acid. When concentrated hydrochloric acid reacts with magnesium, it produces magnesium chloride and hydrogen gas more quickly and vigorously compared to when dilute hydrochloric acid reacts with magnesium. This is due to the higher concentration of hydrogen ions in concentrated hydrochloric acid, leading to a faster and more intense reaction.
Exothermic reaction