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Problem: Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is2 Mg(s) + O2(g) → 2 MgO(s)When 10.1 g Mg is allowed to react with 10.5 g O2, 12.0 g MgO is collected.Determine the theoretical yield for the reaction.

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2 Mg(s) + O2(g) → 2 MgO(s)


Calculate the amount of MgO produced from each reactant and determine the limiting reactant:

mass Mg (molar mass) → moles Mg (mole-to-mole comparison) → moles MgO (molar mass) → mass MgO 

molar mass Mg = 24.305 g/mol
molar mass MgO = 40.305 g/mol

mass MgO=10.1 g Mg×1 mol Mg24.305 g Mg×2 mol MgO2 mol Mg×40.305 g MgO1 mol MgO

mass MgO = 16.75 g MgO


mass O2 (molar mass) → moles O2 (mole-to-mole comparison) → moles MgO (molar mass) → mass MgO 

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Problem Details

Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is

Mg(s) + O2(g) → 2 MgO(s)

When 10.1 g Mg is allowed to react with 10.5 g O2, 12.0 g MgO is collected.

Determine the theoretical yield for the reaction.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.