How many grams of magnesium oxide are produced when 40 grams of oxygen react with magnesium
Follow the steps in this example.
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To determine the number of grams of magnesium oxide produced when 40 grams of oxygen react with magnesium, we need to use the balanced chemical equation for the reaction. The balanced equation for the reaction between magnesium and oxygen to form magnesium oxide is:
2 Mg + O2 -> 2 MgO
From the balanced equation, we can see that 2 moles of Mg react with 1 mole of O2 to produce 2 moles of MgO. To find the amount of magnesium oxide produced, we can follow these steps:
Step 1: Convert the given mass of oxygen to moles.
To do this, we need to know the molar mass of oxygen, which is approximately 16 grams per mole. We can set up the following conversion:
40 grams O2 * (1 mole O2 / 32 grams O2) = 1.25 moles O2
Step 2: Determine the mole ratio between oxygen and magnesium oxide.
From the balanced equation, we know that 1 mole of O2 reacts with 2 moles of MgO. Therefore, we can set up the following conversion:
1.25 moles O2 * (2 moles MgO / 1 mol O2) = 2.5 moles MgO
Step 3: Convert moles of magnesium oxide to grams.
To do this, we need to know the molar mass of magnesium oxide, which is approximately 40 grams per mole. We can set up the following conversion:
2.5 moles MgO * (40 grams MgO / 1 mole MgO) = 100 grams MgO
Therefore, when 40 grams of oxygen react with magnesium, approximately 100 grams of magnesium oxide are produced.