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AleksAgata [21]
3 years ago
5

Two moles of magnesium (Mg) and five moles of oxygen (O2) are placed in a reaction vessel. When magnesium is ignited, it reacts

with oxygen. What is the limiting reactant in this experiment?
Mg + O2 → MgO (unbalanced)

A.
Mg

B.
O2

C.
MgO

D.
both the reactants are in same proportion
Chemistry
1 answer:
SOVA2 [1]3 years ago
6 0

Answer:

\boxed{\text{Mg is the limiting reactant}}

Explanation:

We are given the amounts of two reactants, so this is a limiting reactant problem.

We know that we will need moles, so, lets assemble the data in one place.

           2Mg + O₂ ⟶ 2MgO

n/mol:    2       5

Calculate the moles of MgO we can obtain from each reactant.

From Mg:  

The molar ratio of MgO:Mg is 2:2

\text{Moles of MgO} = \text{2 mol Mg} \times \dfrac{\text{2 mol MgO}}{\text{2 mol Mg}} = \text{2 mol MgO}

From O₂:  

The molar ratio of MgO:O₂ is 2:1.

\text{Moles of MgO} = \text{5 mol O}_{2} \times \dfrac{\text{2 mol MgO}}{\text{1 mol O}_{2}} = \text{10 mol MgO}\\\\\boxed{\textbf{Mg is the limiting reactant}} \text{ because it gives the smaller amount of MgO}

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