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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 is2Mg(s) + O2(g) → 2MgO(s)When 10.1 g Mg is allowed to react with 10.5 g O2, 12.0 g MgO is collected.Determine the percent yield for the reaction.

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We are asked to determine the percent yield for the reaction.


2Mg(s) + O2(g) → 2MgO(s)


Molar Mass Mg = 24.31 g/mol

Molar Mass O2 = 32.00 g/mol

Molar Mass MgO = 40.31 g/mol


Calculate MgO using both reactants: 

10.1 g Mg × 1 mol Mg 24.31 g Mg ×2  mol MgO 2 mol Mg ×40.31 g1 mol MgO  = 16.75 g MgO10.5 g O2 × 1  mol O232.0 g O2 ×2  mol MgO 1 mol O2×40.31 g1 mol MgO  = 26.45 g 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

2Mg(s) + O2(g) → 2MgO(s)

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

Determine the percent yield for the reaction.

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