Final answer:
To calculate the maximum mass of sulfur dioxide produced, we need to convert the mass of carbon disulfide and oxygen to moles, identify the limiting reagent, and then use stoichiometry to find the mass of SO2 that can be produced.
Step-by-step explanation:
The question asks for the maximum mass of sulfur dioxide (SO2) that can be produced from the reaction of 95.6 g of carbon disulfide (CS2) with 100.0 g of oxygen (O2). To solve this, we start by converting the given mass of CS2 to moles using its molar mass and then use the balanced chemical equation to find the moles of SO2 that can be produced. The equation for this reaction is:
CS2 + 3O2 → CO2 + 2SO2.
By converting the respective masses of CS2 and O2 to moles, we can identify which reactant is the limiting reagent and thus calculate the maximum amount of SO2 that can be formed. The molar masses are 76.14 g/mol for CS2 and 32.00 g/mol for O2. The molar mass for SO2 is 64.06 g/mol, which is needed to convert moles of SO2 back to grams.
Moles of CS2 = mass of CS2 / molar mass of CS2Moles of O2 = mass of O2 / molar mass of O2
Once the limiting reagent is identified, we can calculate the moles of SO2 produced by using the stoichiometric coefficients from the balanced equation, then convert the moles of SO2 to grams.