Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg (s) + O₂(g) - 2MgO (s)
How many moles of O₂are consumed when 0.770 mol of magnesium burns?

Question

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O₂(g) - 2MgO (s) How many moles of O₂are consumed when 0.770 mol of magnesium burns?

Quizplus · Accepted Answer

From the balanced chemical equation, we can see that the coefficient of O₂ is 1, which means that 1 mole of O₂ is consumed for every 2 moles of Mg. Therefore, if 0.770 mol of Mg is consumed, we can calculate the moles of O₂ using dimensional analysis: 0.770 mol Mg x (1 mol O₂/2 mol Mg) = 0.385 mol O₂ Therefore, the answer is B.

Magnesium Burns in Air with a Dazzling Brilliance to Produce