Final answer:
To find the theoretical yield of CO2, calculate the number of moles of C6H6 from the given mass and its correct molar mass, then use stoichiometry to determine the moles and mass of CO2. The calculation yields 197.15 g of CO2, but this doesn't match any of the provided answer choices.
Step-by-step explanation:
The question involves the combustion of benzene (C6H6) and the calculation of the theoretical yield of CO2 produced, hence it pertains to stoichiometry and chemical reactions in chemistry.
First, we calculate the number of moles of C6H6 using the given mass (175 g) and its molar mass (78.11 g/mol, corrected for benzene):
Number of moles = Mass / Molar mass = 175 g / 78.11 g/mol = 2.240 moles
From the balanced chemical equation, 2 moles of C6H6 produce 4 moles of CO2. Therefore, using stoichiometry:
Moles of CO2 produced = (2.240 moles C6H6 / 2) * 4 = 4.480 moles CO2
To find the mass of CO2 produced:
Mass of CO2 = Moles of CO2 * Molar mass of CO2 = 4.480 moles * 44.01 g/mol = 197.15 g CO2
However, none of the provided answer choices (240.04 g, 320.06 g, 440.08 g, 480.12 g) matches the calculated result, indicating that either there is an error in the provided answer choices or in the initial data provided such as the molar mass of C6H6.