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Magnesium burns in excess oxygen to form magnesium oxide. The balanced equation for this reaction...

Question:

Magnesium burns in excess oxygen to form magnesium oxide.

The balanced equation for this reaction is:

{eq}2Mg + O_2 \to 2MgO {/eq}.

Starting with 1.35 g of magnesium, calculate the maximum mass of magnesium oxide that could be formed in this reaction.

(relative atomic masses: {eq}O {/eq} = 16.0 g/mol, {eq}Mg {/eq} = 24.0 g/mol)

Maximum Product Obtainable:

The maximum product obtainable is the same quantity that we typically calculate in most limiting reagent problems in a chemical reaction. The maximum product obtainable is a theoretical construct that assumes 100 percent yield, which is an impossibility in the real world.

Answer and Explanation:

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First, we will calculate the number of moles of magnesium present:

$$\begin{align}\\ \text{moles of Mg}&=\frac{\rm Mass\; of\; Mg}{\rm Atomic\;...

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Calculating Reaction Yield and Percentage Yield from a Limiting Reactant

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Chapter 9 / Lesson 6
54K

How to calculate the theoretical yield? Learn the definition and formula of percent yield. Use the theoretical yield equation to calculate theoretical yield.


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