Question

Calculate the volume occupied by 4.4 g of CO$_2$ gas at 27°C and 1 atm pressure. (\( R = 0.0821 \, \text{L-atm/mol-K} \), Molar mass of CO$_2$ = 44 g/mol)

• A. 2.46 L
• B. 1.68 L
• C. 4.48 L
• D. 5.6 L

Hint:

Use the ideal gas law \( PV = nRT \) to find the volume of a gas. Convert temperature to Kelvin and ensure units are consistent.

Answer 1

The Correct Option is A

- Use the ideal gas law: \( PV = nRT \). - Given: Mass of \( \text{CO}_2 \) = 4.4 g, molar mass = 44 g/mol, \( P = 1 \, \text{atm} \), \( T = 27^\circ\text{C} = 27 + 273 = 300 \, \text{K} \), \( R = 0.0821 \, \text{L-atm/mol-K} \). - Moles of \( \text{CO}_2 \): \[ n = \frac{\text{mass}}{\text{molar mass}} = \frac{4.4}{44} = 0.1 \, \text{mol} \] - Solve for volume \( V \): \[ V = \frac{nRT}{P} = \frac{0.1 \times 0.0821 \times 300}{1} = 0.1 \times 0.0821 \times 300 = 2.463 \, \text{L} \]