Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg(s)+ $\mathrm { O } _ { 2 }$ (g)? 2MgO(s)
How many moles of $\mathrm { O } _ { 2 }$ are consumed when 0.850 mol of magnesium burns?

Question

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 
2Mg(s)+ $\mathrm { O } _ { 2 }$ (g)? 2MgO(s)
How many moles of $\mathrm { O } _ { 2 }$ are consumed when 0.850 mol of magnesium burns?

Quizplus · Accepted Answer

According to the balanced equation, 2 moles of Mg react with 1 mole of O2. Therefore, 0.850 moles of Mg will react with 0.425 moles of O2.

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 $\mathrm { O } _ { 2 }$