What is the density (in g/L) of carbon dioxide gas at STP, given that the molar volume of a gas at STP is 22.4 L/mol?

• A. 2.00 g/L
• B. 2.20 g/L
• C. 1.96 g/L
• D. 1.98 g/L

Answer: (D)

Verified step by step guidance

1. First, understand that STP (Standard Temperature and Pressure) conditions are defined as 0°C (273.15 K) and 1 atm pressure. Under these conditions, the molar volume of any ideal gas is 22.4 L/mol.
2. Next, identify the molar mass of carbon dioxide (CO₂). Carbon dioxide consists of one carbon atom and two oxygen atoms. The atomic mass of carbon is approximately 12.01 g/mol, and the atomic mass of oxygen is approximately 16.00 g/mol.
3. Calculate the molar mass of CO₂ by adding the atomic masses: \( \text{Molar mass of CO}_2 = 12.01 \text{ g/mol} + 2 \times 16.00 \text{ g/mol} = 44.01 \text{ g/mol} \).
4. To find the density of CO₂ at STP, use the formula for density: \( \text{Density} = \frac{\text{Mass}}{\text{Volume}} \). Here, the mass is the molar mass of CO₂, and the volume is the molar volume at STP.
5. Substitute the values into the density formula: \( \text{Density} = \frac{44.01 \text{ g/mol}}{22.4 \text{ L/mol}} \). This will give you the density of CO₂ in g/L.