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Magnesium burns: 2Mg + O₂ → 2MgO. A jar holds 6.0 g of oxygen, and 6.0 g of magnesium ribbon burns…

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Magnesium burns: $2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO}$ . A jar holds $6.0\ \text{g}$ of oxygen, and $6.0\ \text{g}$ of magnesium ribbon burns in it. Find the limiting reagent, the mass of magnesium oxide and the oxygen left. Use Mg $= 24.31$ , $\text{O}_2 = 32.00$ and MgO $= 40.31$ g/mol.

Need a reminder? The key ideaShow

Rounds of the equation for a reactant $= \dfrac{\text{moles}}{\text{coefficient}}$ . The smallest is the extent, and its reactant is limiting. Products: extent $\times$ coefficient. Excess left: moles $-$ extent $\times$ coefficient. Percent yield $= \dfrac{\text{actual}}{\text{theoretical}} \times 100$ . At STP a mole of gas fills $22.7\ \text{L}$ .

The worked solution

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Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.

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