Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2 Mg(s) + O₂(g) → 2 MgO(s)
When 4.00 g of magnesium burns,what is the theoretical yield of magnesium oxide?

Question

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+ O₂(g)→ 2 MgO(s) When 4.00 g of magnesium burns,what is the theoretical yield of magnesium oxide?

Quizplus · Accepted Answer

To find the theoretical yield, we need to use stoichiometry. The balanced equation tells us that 2 moles of Mg react with 1 mole of O2 to produce 2 moles of MgO. Using the molar mass of Mg (24.31 g/mol), we can convert the given mass to moles:

4.00 g Mg x (1 mol Mg/24.31 g Mg) = 0.165 mol Mg

Since the reaction ratio is 2:2, the number of moles of MgO produced will be the same as the number of moles of Mg. We can then convert this to mass using the molar mass of MgO (40.30 g/mol):

0.165 mol MgO x (40.30 g MgO/1 mol MgO) = 6.63 g MgO

Therefore, the theoretical yield of MgO is 6.63 g.

Magnesium Burns in Air with a Dazzling Brilliance to Produce