# 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 | 2H_{2}(g) | + | O_{2}(g) | → | 2H_{2}O (l) |

Molecules | 2 Molecules H_{2} | + | 1 molecule O_{2} | → | 2 molecules H_{2}O |

Amount (mol): | 2 mols H_{2} | + | 1 mol O_{2} | → | 2 mols H_{2}O |

This is a balanced equation, hence we can say, 2 mol of H_{2} are equivalent to 1 mol of O_{2}, and to 2 mol of H_{2}O

Based on these equivalences, we can say that:

- Two mol of H
_{2} are needed to produce 2 mol of H_{2}O
- One mol of O
_{2} is needed to produce 2 mol of H_{2}O
- Two mol of H
_{2} are needed for each 1 mol of O_{2} to produce 2 mol of H_{2}O

**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