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Answer :
Final answer:
When 32.1 g of sulfur burns, it will produce approximately 98.1 g of sulfuric acid, according to the stoichiometry of the balanced reactions.
Explanation:
When sulfur burns, it reacts with oxygen to form sulfur dioxide (SO2), which further reacts with oxygen to form sulfur trioxide (SO3). The sulfur trioxide then reacts with water to produce sulfuric acid (H2SO4) as part of a series of reactions. The balanced chemical equations for these reactions are:
- S + O2 → SO2
- 2SO2 + O2 → 2SO3
- SO3 + H2O → H2SO4
To find out how many grams of sulfuric acid are produced from 32.1 g of sulfur, you need to calculate using stoichiometry based on these equations. The molar mass of sulfur is approximately 32.1 g/mol, and the molar mass of sulfuric acid is approximately 98.1 g/mol. Therefore, for every one mole of sulfur that burns, one mole of H2SO4 will be produced, which equates to 98.1 g of H2SO4. So, if you start with 32.1 g of sulfur, you should end up with approximately 98.1 g of sulfuric acid (option b).
Learn more about Stoichiometry here:
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