Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg(s)+ $\mathrm { O } _ { 2 }$ (g)? 2MgO(s)
When 6.00 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: 
2Mg(s)+ $\mathrm { O } _ { 2 }$ (g)? 2MgO(s)
When 6.00 g of magnesium burns,what is the theoretical yield of magnesium oxide?

Quizplus · Accepted Answer

The molar mass of Mg is 24.31 g/mol, and the molar mass of MgO is 40.31 g/mol. For 6.00 g of Mg, the moles are 6.00 g / 24.31 g/mol = 0.247 mol. The reaction shows a 1:1 molar ratio, so 0.247 mol of Mg produces 0.247 mol of MgO. The mass of MgO is 0.247 mol * 40.31 g/mol = 9.95 g.

Magnesium Burns in Air with a Dazzling Brilliance to Produce O2\mathrm { O } _ { 2 }O2​

Magnesium Burns in Air with a Dazzling Brilliance to Produce $\mathrm { O } _ { 2 }$