Respuesta :
Answer:
If a sample of 2 moles of nitric oxide gas was reacted with excess oxygen, 2 moles of nitrogen dioxide would be produced.
Explanation:
The balanced reaction is:
2 NO + O₂ → 2 NO₂
By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of each compound participate in the reaction:
- NO: 2 moles
- O₂: 1 mole
- NO₂: 2 moles
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop.
The limiting reagent is one that is consumed first in its entirety, determining the amount of product in the reaction. When the limiting reagent is finished, the chemical reaction will stop. By reaction stoichiometry, if a sample of 2 moles of nitric oxide gas was reacted with excess oxygen, 2 moles of nitrogen dioxide would be produced.
Excess reagents are reactants that do not completely vanish after the reaction is complete. Moles of nitrogen dioxide produced is 2 moles.
What is limiting and excess reagents?
In a chemical reaction when the reactant is left and is not completely consumed after the formation of the product is called excess reagents.
The reactants or the reagents that get consumed first in the reaction and limit the product formation is called limiting reagent.
The balanced chemical reaction can be shown as,
[tex]\rm 2NO + O_{2} \rightarrow 2NO_{2}[/tex]
The stoichiometry coefficient gives the moles of the reactant and the products as,
- Moles of nitric oxide = 2 moles
- Moles of oxygen = 1 mole
- Moles of nitrogen dioxide = 2 moles
According to the reaction if the 2 moles of nitric oxide reacts with an excess of the oxygen gas then 2 moles of [tex]\rm NO_{2}[/tex] is produced.
Therefore, moles of nitrogen dioxide produced is 2 moles.
Learn more about limiting and excess reagent here:
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