Quantitative Information from Balanced Equations

Introduction

Remark: In a balanced equation, reactants and products are equivalent to each other.

Example

**Information from Balanced Equations**
Equation	2H₂(g)	+	O₂(g)	→	2H₂O (l)
Molecules	2 Molecules H₂	+	1 molecule O₂	→	2 molecules H₂O
Amount (mol):	2 mols H₂	+	1 mol O₂	→	2 mols H₂O

This is a balanced equation, hence we can say, 2 mol of H₂ are equivalent to 1 mol of O₂, and to 2 mol of H₂O

Based on these equivalences, we can say that:

Two mol of H₂ are needed to produce 2 mol of H₂O
One mol of O₂ is needed to produce 2 mol of H₂O
Two mol of H₂ are needed for each 1 mol of O₂ to produce 2 mol of H₂O

Hence, if # mol of any reactant is known, # mol of the product can be calculated as long as both are represented in a balanced equation.

Note:
A balanced equation contains the correct # mol for each of the reactants and products.
If their masses (in grams) were given instead, these should be converted into mol using the conversion equation between them.

Exercise

Exercise on Mass Produced from Burning Butane

Check your answers here: Solution to the Exercise on Mass Produced from Burning Butane

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Date of last modification: Summer , 2019