Consider the reaction below, if 5 moles each of hydrogen and oxygen are reacted to form water, the reaction reveals? 2H2 + O2 __> 2H2O

A. H2 is excess reagent
B. O2 is limiting reagent
C. H2 is limiting reagent
D. Reaction has no limiting reagent


Correct Answer: D. Reaction has no limiting reagent

Detail about MCQs

To determine which reactant is the limiting reagent and which is in excess, we need to compare the mole ratios of hydrogen (H2) and oxygen (O2) in the balanced chemical equation to the actual moles of each reactant given:
Balanced equation: 2H2 + O2 → 2H2O
From the balanced equation, we can see that the stoichiometric ratio of H2 to O2 is 2:1.
Now, you have 5 moles each of hydrogen and oxygen:
• Moles of H2 = 5 moles
• Moles of O2 = 5 moles The mole ratio of H2 to O2 in the given reactants is 5:5, which simplifies to 1:1. Since the actual ratio of moles (1:1) matches the stoichiometric ratio (2:1) in the balanced equation, it means that there are enough moles of both hydrogen and oxygen to react completely without either being in excess or limiting. Therefore, the correct answer is:

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