Answer :
Final answer:
This specific stoichiometry problem falls under the category of Chemistry involves calculating the mass of sulfur produced through a chemical reaction involving H2S and SO2. The relationship between the components in the reaction is established by first converting the given masses into moles, then applying the ratios from the balanced equation.
Explanation:
The subject of this question falls under the category of Chemistry as it is dealing with chemical reactions. The provided equation isn't clear, but let's assume you are asking about a reaction where H2S and SO2 are combining to produce sulfur (S) and water. This is a stoichiometry problem, which is based on the law of conservation of mass.
A balanced equation for this reaction might be: 2H2S (g) + SO2(g) = 3S(s) + 2H2O(g). This means that, in a perfect scenario, two moles of H2S react with one mole of SO2 to produce three moles of sulfur and two moles of water.
To find out how many grams of sulfur can be produced we need to calculate using moles and molar mass of the components. Based on molar masses (S=32.1 g/mol, H=1.01 g/mol, and O=16.0 g/mol), the molar mass of H2S = 34.1 g/mol and SO2 = 64.1 g/mol. Therefore, if we take 12.6 g of H2S, it corresponds to 12.6 / 34.1 = 0.37 moles of H2S. Similarly, 14.6 g of SO2 corresponds to 14.6 / 64.1 = 0.23 moles of SO2.
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