Question

what is the density of co₂ gas at stp?
○ 4.41 g/l
○ 1.20 g/l
○ 1.96 g/l
○ 8.21 g/l
○ 2.73 g/l

Explanation:

Step1: Recall molar mass of CO₂

Molar mass of C is 12.01 g/mol, O is 16.00 g/mol. So \( M = 12.01 + 2\times16.00 = 44.01 \, \text{g/mol} \).

Step2: Use STP volume

At STP, 1 mole of gas occupies \( 22.4 \, \text{L} \).

Step3: Calculate density

Density \(
ho = \frac{M}{V_m} \), where \( V_m = 22.4 \, \text{L/mol} \). So \(
ho = \frac{44.01 \, \text{g/mol}}{22.4 \, \text{L/mol}} \approx 1.96 \, \text{g/L} \)? Wait, no, wait: Wait, 44.01 / 22.4 ≈ 1.96? Wait, no, 44 divided by 22.4 is approximately 1.96? Wait, no, 44/22.4 ≈ 1.96? Wait, no, 44.01/22.4 ≈ 1.96? Wait, no, wait, maybe I miscalculated. Wait, 44.01 divided by 22.4: 22.41.96 = 22.42 - 22.40.04 = 44.8 - 0.896 = 43.904, which is close to 44.01. Wait, but wait, the options: 4.41? Wait, no, maybe I messed up. Wait, no, density is mass per volume. At STP, 1 mole of CO₂ is 44.01 g, and volume is 22.4 L. So 44.01 g / 22.4 L ≈ 1.96 g/L? Wait, but the first option is 4.41. Wait, no, wait, maybe I made a mistake. Wait, no, 44.01 / 22.4 ≈ 1.96? Wait, no, 22.42 = 44.8, so 44.01 is less than 44.8, so 44.01/22.4 ≈ 1.96. Wait, but the options have 1.96 as an option. Wait, but let me check again. Molar mass of CO₂: C=12.01, O=16.00*2=32.00, total 44.01 g/mol. STP volume: 22.4 L/mol. So density = 44.01 g/mol / 22.4 L/mol ≈ 1.96 g/L. So the correct option is 1.96 g/L. Wait, but the first option is 4.41. Wait, no, maybe I confused with another formula. Wait, no, density is mass over volume. So 44 g / 22.4 L ≈ 1.96 g/L. So the answer should be 1.96 g/L.

Answer:

1.96 g/L (the option with 1.96 g/L)