Question

What volume of O2(g) is required to react with excess CS2(l) to produce 4.0 L of CO2(g)? (Assume all gases are measured at 0°C and 1 atm.)

Answer 1

To produce 4.0 L of CO₂(g), 12.0 L of O₂(g) would be required to react with excess CS₂(l) based on the stoichiometric relationship derived from the balanced chemical equation and Avogadro's law.

Step-by-step explanation:

To determine the volume of O₂(g) required to react with excess CS₂(l) to produce 4.0 L of CO₂(g), we need to refer to the balanced chemical equation:

CS₂(l) + 3O₂(g) → CO₂(g) + 2SO₂(g)

From this equation, we can see that 1 mole of CS₂ reacts with 3 moles of O₂ to produce 1 mole of CO₂. Since we are dealing with volumes of gases at the same conditions of temperature and pressure (0°C and 1 atm), we can use the direct relationship between moles and volumes provided by Avogadro's law, which states that equal volumes of gases at the same temperature and pressure contain equal numbers of moles.
Therefore, if producing 1 volume of CO₂ requires 3 volumes of O₂, producing 4.0 L of CO₂ would require:

4.0 L CO₂ × 3 L O₂ / 1 L CO₂ = 12.0 L O₂

Thus, 12.0 L of O₂(g) would be required to react with excess CS₂(l) to produce 4.0 L of CO₂(g) under the stated conditions.