SUMMARY
The discussion centers on calculating the mass of gold (Au) produced from the complete reduction of 0.0500 mol of gold(III) sulfide (Au2S3) using excess hydrogen (H2). The participant initially calculated the mass as 19.7 grams based on the molar mass of gold (197 g/mol) but questioned the accuracy of this result after finding it inconsistent with a textbook answer. The correct approach confirms that 19.7 grams is indeed the accurate mass of Au produced from the given amount of Au2S3.
PREREQUISITES
- Understanding of stoichiometry in chemical reactions
- Familiarity with molar mass calculations
- Knowledge of reduction reactions involving metals
- Basic principles of chemical equations
NEXT STEPS
- Review stoichiometric calculations for reduction reactions
- Study the properties and reactions of gold(III) sulfide (Au2S3)
- Learn about the molar mass of common elements and compounds
- Explore the principles of using excess reactants in chemical reactions
USEFUL FOR
Chemistry students, educators, and anyone involved in chemical calculations or stoichiometry, particularly in the context of metal reduction reactions.