Q. 7.111 - An Introduction to General, Organic, and Biological Chemistry

Question

Consider the following unbalanced equation: 

$\mathrm{Al}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)$

1.  Write the balanced chemical equation. 
2.  Identify the type of reaction. 
3.  How many moles of ${\mathrm{O}}_2$ are needed to react with $4.50$ moles of $\mathrm{Al}$ ?
4.  How many grams of ${\mathrm{Al}}_2{\mathrm{O}}_3$ are produced when $50.2 g$ of $\mathrm{Al}$ reacts?
5. When $\mathrm{Al}$ is reacted with $8.00 g$ of ${\mathrm{O}}_2$, how many grams of ${\mathrm{Al}}_2{\mathrm{O}}_3$ can form? 

Step-by-Step Solution

Answer

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Part (a) Step 1: Given Information

We need to balance equation: $\mathrm{Al}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)$

Step 2: Explanation

To balance an equation we need the number of atoms of each element is the same on both sides of the equation.  Representing it in table form:

Reactant	Product
$1 \mathrm{Al}$	$2 \mathrm{Al}$	Unbalanced
$2 \mathrm{O}$	$3 \mathrm{O}$	Unbalanced