If 4 moles of hydrogen react with 4 moles of oxygen which of these is the limiting reagent?
2(H2) + O2 --> 2(H2O)
You can see in the reaction that two moles of hydrogen react with two moles of oxygen.
So if you have the save amount of both, which will finish first? So which is the limiting reagent?
*one mole of oxygen
Hydrogen?....
four moles of H2 needs 2 moles of O2, so you have more O2 than needed **fourmoles***, so H2 is the limiting reaction, and it runs out first.
i have another question that goes to this one can you help me? It says
What is the maximum amount of water (in grams) that can be produced give it for most of hydrogen and for most of oxygen?
I have no idea what "most" means.
if the limiting reagent is hydrogen, then four moles of H2 yields four moles of H2O
To determine the limiting reagent in a chemical reaction, you need to compare the stoichiometric ratios of the reactants.
In this case, we have 4 moles of hydrogen and 4 moles of oxygen. The balanced chemical equation for the reaction between hydrogen (H₂) and oxygen (O₂) is:
2H₂ + O₂ → 2H₂O
From the equation, we can see that the stoichiometric ratio between hydrogen and oxygen is 2:1. That means it takes 2 moles of hydrogen to react with 1 mole of oxygen.
Since we have 4 moles of hydrogen and 4 moles of oxygen, we can calculate the amount of oxygen needed to react with the available hydrogen.
4 moles of hydrogen × (1 mole of oxygen / 2 moles of hydrogen) = 2 moles of oxygen required
Comparing the required amount of oxygen (2 moles) with the available amount of oxygen (4 moles), we can conclude that 2 moles of oxygen is the limiting reagent.
The limiting reagent is the reactant that is completely consumed first and limits the amount of product that can be formed. In this case, since we have fewer moles of oxygen than are required to react with the available hydrogen, oxygen is the limiting reagent.