# 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.

###### FREE Expert Solution

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:

85% (234 ratings) ###### 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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