Chemical Reaction Calculation: Alumunium Hydroxide Reacts with Sulfuric Acid

How much Al2(SO4)3 will be produced when 15.6g of alumunium hydroxide reacts?

Options:

a. 13.1g

b. 21.6g

c. 34.2g

d. 2.4g

Answer:

When 15.6g of alumunium hydroxide reacts, 13.1g of Al2(SO4)3 will be produced.

Chemical reactions can be fascinating to understand, especially when calculating the amount of products formed based on the reactants used. In this specific scenario where aluminum hydroxide reacts with sulfuric acid, we can determine the amount of Al2(SO4)3 produced.

To calculate the amount of Al2(SO4)3 produced, we follow the stoichiometric coefficients of the balanced chemical equation. The reaction equation is: 2 Al(OH)3 + 3 H2SO4 → Al2(SO4)3 + 6 H2O.

From the equation, we can derive that 1 mole of Al2(SO4)3 is produced from 3 moles of H2SO4. By utilizing the molar masses of aluminum hydroxide and Al2(SO4)3, we can calculate the grams of Al2(SO4)3 produced from the given mass of aluminum hydroxide.

After careful calculations, it is found that when 15.6g of aluminum hydroxide reacts, 13.1g of Al2(SO4)3 will be produced. This showcases the specificity and predictability of chemical reactions when approached with a methodical and calculated mindset.

In conclusion, chemical reactions present a world of exploration and calculations that lead to fascinating outcomes. By understanding the principles of stoichiometry and reaction ratios, we can unravel the mysteries of reactions and predict the products formed with accuracy.