Final answer:
The amount of sulfur required can be determined through stoichiometry which depends on the specific chemical reaction involving hydrogen and sulfur. Without the full details, assuming sulfuric acid formation, 0.366 g of hydrogen would require approximately 2.928 g of sulfur.
Step-by-step explanation:
To determine how many grams of sulfur must be obtained if 0.366 grams of hydrogen is obtained in the experiment, stoichiometry of the reaction needs to be considered. Given that hydrogen and sulfur are part of a compound such as sulfuric acid (H2SO4), we can infer that the chemical reaction is balanced in proportions determined by the molar mass and stoichiometry of the reactants and products.
Considering the information from the example stating that 0.708 grams of elemental sulfur correspond to 0.028 moles of solute, and the molar mass of sulfur is 32 g/mol, we can derive that if hydrogen has a molar mass around 1 g/mol and is present as H2, 0.366 g of hydrogen represents 0.366/2 = 0.183 moles of hydrogen.
Without the full stoichiometry of the reaction, it is not possible to provide an exact mass of sulfur needed. However, for sulfuric acid, where the ratio of hydrogen to sulfur is 2:1 by mole, 0.183 moles of hydrogen would theoretically require 0.0915 moles of sulfur. Using the molar mass of sulfur (32 g/mol) this would equate to 0.0915 moles * 32 g/mol = 2.928 grams of sulfur.