How many moles of CO₂ are produced when 45.0g of C₆H₆ react completely in the following equation? 2C₆H₆ + 15O₂ $\rarr$12CO₂ + 6H₂O

Question

Quizplus · Accepted Answer

First, we need to calculate the molar mass of CS₂O (carbon disulfide). The molar mass of carbon (C) is approximately 12.01 g/mol, and the molar mass of sulfur (S) is approximately 32.07 g/mol. Therefore, the molar mass of CS₂ is 12.01 + (2 * 32.07) = 76.15 g/mol.Given that 45.0 g of CS₂ reacts, we can find the number of moles of CS₂ that react by dividing the mass of CS₂ by its molar mass: 45.0 g / 76.15 g/mol = 0.591 moles of CS₂.According to the balanced chemical equation, 2 moles of CS₂ produce 12 moles of COS. Therefore, 0.591 moles of CS₂ would produce (12/2) * 0.591 = 3.546 moles of COS, which rounds to 3.46 moles when considering significant figures.

How Many Moles of CO2 Are Produced When 45 →\rarr→ 12CO2 + 6H2O A)0

How Many Moles of CO₂ Are Produced When 45 $\rarr$ 12CO₂ + 6H₂O
A)0