Question

Given the following chemical reaction, 2 C₆H₆ + 15 O₂ → 12 CO₂ + 6 H₂O, how many liters of CO₂ will be made if 156 g of C₆H₆ are burned completely with excess oxygen gas?

Answer 1

To find the volume of CO₂ produced from 156 g of C₆H₆, we convert the mass of benzene to moles, use the stoichiometry of the balanced equation, and apply the ideal gas law, yielding 268.8 liters of CO₂.

Step-by-step explanation:

To calculate how many liters of CO₂ are produced when burning 156 g of C₆H₆ with excess oxygen, we start with the chemical reaction: 2 C₆H₆ + 15 O₂ → 12 CO₂ + 6 H₂O. First, we determine the molar mass of benzene (C₆H₆), which is approximately 78.11 g/mol. Next, we convert the mass of C₆H₆ into moles:

156 g C₆H₆ × (1 mol C₆H₆ / 78.11 g C₆H₆) = 2 moles C₆H₆

According to the balanced chemical equation, 2 moles of C₆H₆ yield 12 moles of CO₂. Since the reaction coefficients indicate a direct mole-to-mole ratio, we can directly determine the moles of CO₂:

12 moles CO₂

Finally, we use the ideal gas law which states that at Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 liters. Hence, the volume of CO₂ produced is:

12 moles CO₂ × 22.4 L/mol = 268.8 liters CO₂