Gas density at standard conditions – carbon dioxide Express the density of CO2 at normal conditions as kg per normal cubic meter (kg/Nm^3). Choose the correct expression.

Introduction / Context:Normal cubic meter (Nm^3) refers to gas volume at standard temperature and pressure. Converting molar properties to mass per unit standard volume is a frequent step in gas metering, emissions reporting, and process calculations.

Given Data / Assumptions:

• Molar mass of CO2 = 44 kg/kmol.
• Molar volume at STP (approximately) = 22.4 m^3/kmol (for ideal gas at 0°C, 1 atm).
• Seeking density in kg per Nm^3.

Concept / Approach:Density at STP is mass per mole divided by molar volume. For any gas, ρ = M / V_m, where M is molar mass and V_m is molar volume at the stated standard conditions. For CO2: ρ ≈ 44 kg/kmol / 22.4 m^3/kmol.

Step-by-Step Solution:

Verification / Alternative check:Comparing to air (≈28.97/22.4 ≈ 1.29 kg/Nm^3), CO2's higher density is consistent with its higher molar mass.

Why Other Options Are Wrong:

• 44/22400: Uses liters in the denominator but keeps kg units, giving kg per liter-scale denominator numerically wrong for kg/Nm^3.
• 22.4/44: Inverts the correct ratio, yielding m^3/kg rather than kg/m^3.
• None of these: Incorrect because 44/22.4 is correct.

Common Pitfalls:Mixing L/mol with m^3/mol without consistent unit conversions; forgetting that 1 Nm^3 corresponds to 1 m^3 at standard conditions.

Final Answer:44/22.4