Balanced chemical reaction happening here is:
3Mg(s) + N₂(g) → Mg₃N₂(s)
<u>moles of product formed from each reactant:</u>
2.0 mol of N2 (g) x <u> 1 mol Mg₃N₂ </u> = <u>2 mol Mg₃N₂</u>
1 mol N2
and
8.0 mol of Mg(s) x <u> 1 mol Mg₃N₂ </u> = 2.67 mol Mg₃N₂
3 mol Mg
Since N2 is giving the least amount of product(Mg₃N₂) ie. 2 mol Mg₃N₂
N2 is the limiting reactant here and Mg is excess reactant.
Hence mole of product formed here is 2 mol Mg₃N₂
molar mass of Mg₃N₂
= 3 Mg + 2 N
= 101g/mol
mass of product(Mg₃N₂) formed
= moles x Molar mass
= 2 x 101
= 202g Mg₃N₂
<u>202g of product are formed from 2.0 mol of N2(g) and 8.0 mol of Mg(s).</u>
<u> </u> The following are indicators of chemical changes:
Change in Temperature
Change in Color
Formation of a Precipitate
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They are very stable (not reactive).
This is because their outer shell has a total of 8 valence electrons. All elements strive to get towards a full outer shell, but since these elements already have a full outer shell, they are fairly unreactive.
Disaccharide forms when two monomers join.
