# Question #595a5

May 11, 2017

Did you do this reaction in the lab?

#### Explanation:

I expect that you did, and did you notice the warmth of the reaction flask at the experiment proceeded..........? Again, I think that you did.

The stoichiometric equation is..........

$M g \left(s\right) + 2 H C l \left(a q\right) \rightarrow M g C {l}_{2} \left(a q\right) + {H}_{2} \left(g\right) \uparrow$

Since strong ionic bonds and covalent bonds were formed and (weaker) metallic and covalent bonds broken, the reaction as written is $\text{EXOTHERMIC}$, i.e.

$M g \left(s\right) + 2 H C l \left(a q\right) \rightarrow M g C {l}_{2} \left(a q\right) + {H}_{2} \left(g\right) \uparrow + \Delta$

And we could treat $\Delta$ as an $\text{extensive property.........}$, dependent on the molar quantity of magnesium oxidized. Note that this answer depends on experimental observation.