Aluminum hydroxide reacts with sulfuric acid as follows: $$ 2 \mathrm{Al}(\mathrm{OH})_{3}(s)+3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) $$ Which is the limiting reactant when \(0.500 \mathrm{~mol} \mathrm{Al}(\mathrm{OH})_{3}\) and \(0.500 \mathrm{~mol} \mathrm{H}_{2} \mathrm{SO}_{4}\) are allowed to react? How many moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) can form under these conditions? How many moles of the excess reactant remain after the completion of the reaction?

Understanding stoichiometry is crucial for determining the amounts of substances involved in chemical reactions. This field of chemistry is like a recipe, providing the proportions of reactants needed to produce a specific amount of product.

Imagine you're baking cookies - each ingredient must be added in the right amount. In stoichiometry, we use the 'mole' as the measuring unit, similar to using a cup or tablespoon in baking. By knowing the balanced chemical equation, we can calculate the moles needed or produced of each substance. The equation given in the exercise demonstrates stoichiometry in action, where a specific ratio of reactants yields a set amount of product.

In the exercise, the balanced equation was used to find the limiting reactant and predict the amount of product formed, exemplifying stoichiometry's application. Key to effectively using stoichiometry is starting with a balanced chemical equation, which ensures the law of conservation of mass is followed, meaning all atoms in the reactants will be accounted for in the products.

Chemical reactions are processes where reactants transform into products. Like a dance, atoms in reactants break apart and rearrange to form new substances. It is essential to understand the types of chemical reactions, such as combination, decomposition, single-replacement, double-replacement, and combustion, to predict the products of a reaction.

The exercise showcases a double-replacement reaction where the anions and cations of two compounds switch places. This type of reaction often occurs in aqueous solutions, like the sulfuric acid and aluminum hydroxide reaction provided. Recognizing reaction types helps chemists control and predict the outcomes, ensuring the correct products are formed in the desired quantities. Furthermore, identifying the limiting reactant, the substance that runs out first and stops the reaction, is a crucial aspect of understanding complete chemical reactions.

The mole concept is a bridge between the microscopic world of atoms and the macroscopic world we experience. One mole is defined as the amount of a substance that contains exactly 6.022 x 10²³ particles, which is Avogadro's number. This concept is akin to a dozen eggs - no matter the size of the eggs, a dozen is always twelve. Similarly, a mole of any substance will contain the same number of entities.

In the context of the exercise, understanding the mole concept allowed the calculation of product formed and excess reactant remaining after the chemical reaction. By using the mole ratios provided in the balanced chemical equation, students can convert between moles of different substances. This concept ensures accurate predictions of product amounts and helps in identifying the limiting reactant in a reaction.