10g of Fe produces 14.37g of [tex]Fe_2O_3[/tex] and 7g of [tex]O_2[/tex] produce 46.84g of [tex]Fe_2O_3[/tex]
The limiting reactant (or limiting reagent) is the reactant that gets consumed first in a chemical reaction and therefore limits how much product can be formed
Write the balanced equation for the reaction taking place:
4Fe + 3 [tex]O_2[/tex] ==> 2 [tex]Fe_2O_3[/tex] (rust)
Use the stoichiometry of the balanced equation and dimensional analysis to find limiting reagent & grams of [tex]Fe_2O_3[/tex]:
10 g Fe x 1 mol Fe/55.85 g x 2 mol [tex]Fe_2O_3[/tex]/4 mol Fe x 160 g/mol
[tex]Fe_2O_3[/tex] = 14.37 g [tex]Fe_2O_3[/tex] (2 Significant figures)
7 g [tex]O_2[/tex] x 1 mol [tex]O_2[/tex]/32 g x 2 mol [tex]Fe_2O_3[/tex]/3 mol [tex]O_2[/tex] x 160 g/mol
[tex]Fe_2O_3[/tex] = 46.84 g [tex]Fe_2O_3[/tex] (2 Significant figures)
Hence, 10g of Fe produces 14.37g of [tex]Fe_2O_3[/tex] and 7g of [tex]O_2[/tex] produce 46.84g of [tex]Fe_2O_3[/tex]
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