SUMMARY
The molar ratio for dissolving aluminum with sulfuric acid is established by the balanced chemical equation: 2 Al(s) + 3 H2SO4 → Al2(SO4)3(aq) + 3 H2. This indicates that 3 moles of sulfuric acid are required for every 2 moles of aluminum. To dissolve a 15.2 g aluminum block, one must calculate the minimum mass of H2SO4 needed using the molar masses of aluminum (26.98 g/mol) and sulfuric acid (98.09 g/mol). The correct calculation involves determining the moles of aluminum and applying the molar ratio to find the corresponding mass of sulfuric acid.
PREREQUISITES
- Understanding of stoichiometry
- Familiarity with molar mass calculations
- Knowledge of balanced chemical equations
- Basic algebra for mass and mole conversions
NEXT STEPS
- Calculate the moles of aluminum in 15.2 g
- Determine the mass of sulfuric acid required using the molar ratio
- Review stoichiometric calculations in chemical reactions
- Explore practical applications of sulfuric acid in metal dissolution
USEFUL FOR
Chemistry students, educators, and anyone involved in chemical engineering or laboratory work focusing on acid-base reactions and metal dissolution processes.