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Answer:
3.98 g
Explanation:
Step 1. Write the balanced chemical reaction. In this case, magnesium reacts with oxygen to produce magnesium oxide:
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Step 2. Calculate the number of moles of magnesium:
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Step 3. Calculate the number of moles of oxygen:
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Step 4. Identify the limiting reactant comparing the equivalents. Equivalent of Mg:
Equivalent of oxygen:
Therefore, Mg is the limiting reactant.
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Step 5. According to the stoichiometry of this reaction:
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Step 6. Convert the number of moles of MgO into mass:
I'm assuming that by "miles" you mean moles.
If O2 is the excess reactant, that means Fe is the limiting reactant. That means that the amount of product being formed depends on the amount of Fe reactant present. To calculate the moles of Fe2O3 formed, start with the given 6.4 moles of Fe and use the mole to mole ratio given by the reaction as shown below:
6.4 mol Fe x
= 3.2 mol Fe2O3
If O2 is the excess reactant, that means Fe is the limiting reactant. That means that the amount of product being formed depends on the amount of Fe reactant present. To calculate the moles of Fe2O3 formed, start with the given 6.4 moles of Fe and use the mole to mole ratio given by the reaction as shown below:
6.4 mol Fe x