Question

In a balanced chemical equation, is it true that if both reactants have an equal mass that there will be no limiting reactant? True or False and explain why

Answer 1

This is not true

Step-by-step explanation:

The limiting reactant is described as the reactant in short supply. This indicates that a limiting reactant does not depend on the amount of the reactant given.

The extent to which it is used up in the reaction determines whether a reactant is limiting or not.

For example;

2H₂ + O₂ → 2H₂O

The equation above is balanced.

Lets say 20mole of H₂ reacted with 20mole of O₂

According to the statement in the problem, since the equation is balanced and we have equal number of reactants, then there is no limiting reactant.

This is false

2 mole of H₂ reacted with 1 mole of O₂

20 mole of H₂ will require
`(20)/(2)` moles of O₂ = 10 mole of O₂

But we were given 20 moles of O₂. We see that O₂ is in excess and H₂ is the limiting reactant.