Respuesta :
First off, the chemical equation needs to be balanced. Since there are 2 oxygen atoms in the reactants, we must produce 2 moles of MgO, which means we need 2 moles of Mg, giving:
2Mg + O2 --> 2MgO
Therefore for a stoichiometric reaction where no reactant is left over, the number of moles of magnesium must be double that of oxygen. However, as seen, the molar ratio of magnesium to oxygen is 2:5, meaning oxygen is in large excess, and Magnesium is the limiting reactant. Therefore the answer is A.
2Mg + O2 --> 2MgO
Therefore for a stoichiometric reaction where no reactant is left over, the number of moles of magnesium must be double that of oxygen. However, as seen, the molar ratio of magnesium to oxygen is 2:5, meaning oxygen is in large excess, and Magnesium is the limiting reactant. Therefore the answer is A.
Mg (Magnesium) is the limiting reactant in this experiment. Hence, option A is correct.
What is limiting reagent?
Limiting reagent is the substance that is totally consumed when the chemical reaction is complete.
The amount of product formed is limited by this limited reagent so the reaction cannot continue without it.
Example: If in 18 mole oxygen are present, there would be an excess of (18 - 11.25) = 6.75 mole of unreacted oxygen.
When all the benzene is consumed (Benzene is a limiting reagent).
Chemical Reaction: 2Mg + O2 → 2MgO (Balanced equation)
When Magnesium is react with oxygen in ignited form to produce magnesium oxide (MgO).
Once there is no more of that reactant the reaction cannot proceed therefore hit limits the reaction from continuing.
The excess reagent is the reactant that could keep reacting if the other had not been consumed.
Mg (Magnesium) is the limiting reactant in this experiment. Hence, option A is correct.
Learn more about limiting reagent, Hence:
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