How do i get the mass of magnesium oxide based on this question?

To answer questions like this, you must start with a balanced chemical equation: 2 Mg + O2 --> 2 MgO Calculate how many moles of MgO you can form from the amount of Mg you are given: 0.24 g / 24.3 g --> 0.01 mol Mg X ( 1 mol MgO/1 mol Mg) = 0.01 mol MgO 0.25 mol O2 ( 2 mol MgO / 1 mol O2) = 0.50 mol MgO Since the amount of magnesium will allow you to form less MgO than the amount of oxygen you are given, this reaction can form ONLY 0.01 mol of MgO. The mass of MgO is: 0.01 mol MgO X 40 g MgO/1 mol = 0.4 grams MgO

Magnesium is the limiting reactant (i.e. there is not enough Mg to react with all of the oxygen that is present.) First write the balanced equation for the reaction: 2 Mg + O2 --------> 2 MgO 0.24g Mg x 1 mol Mg/24g Mg x 2 mol MgO /2 mol Mg x 40.0 g MgO / 1 mol MgO = 0.40 g MgO

Magnesium is the limiting reactant (i.e. there is not enough Mg to react with all of the oxygen that is present.) First write the balanced equation for the reaction: 2 Mg + O2 --------> 2 MgO 0.24g Mg x 1 mol Mg/24g Mg x 2 mol MgO /2 mol Mg x 40.0 g MgO / 1 mol MgO = 0.40 g MgO

To answer questions like this, you must start with a balanced chemical equation: 2 Mg + O2 --> 2 MgO Calculate how many moles of MgO you can form from the amount of Mg you are given: 0.24 g / 24.3 g --> 0.01 mol Mg X ( 1 mol MgO/1 mol Mg) = 0.01 mol MgO 0.25 mol O2 ( 2 mol MgO / 1 mol O2) = 0.50 mol MgO Since the amount of magnesium will allow you to form less MgO than the amount of oxygen you are given, this reaction can form ONLY 0.01 mol of MgO. The mass of MgO is: 0.01 mol MgO X 40 g MgO/1 mol = 0.4 grams MgO

Mg + O2 ---> MgO Mass of magnesium + Mass of oxygen --------> Mass of magnesium oxide 0.24g + 4g ----> 4.24g