Question

dry ice is solid carbon dioxide. a 1.87 g sample of dry ice is placed in an evacuated 4.27 l vessel at 24.0 °c. calculate the pressure inside the vessel after all the dry ice has been converted to co₂ gas. round your answer to 3 significant digits. note: reference the fundamental constants table for additional information.

Explanation:

Step1: Calculate moles of CO₂

Molar mass of CO₂ = 12.01 + 2×16.00 = 44.01 g/mol
Moles \( n = \frac{1.87\ \text{g}}{44.01\ \text{g/mol}} \approx 0.04249\ \text{mol} \)

Step2: Convert temperature to Kelvin

\( T = 24.0^\circ\text{C} + 273.15 = 297.15\ \text{K} \)

Step3: Apply ideal gas law \( PV = nRT \)

Rearrange for \( P = \frac{nRT}{V} \), \( R = 0.0821\ \text{L·atm/(mol·K)} \)
\( P = \frac{0.04249\ \text{mol} \times 0.0821\ \text{L·atm/(mol·K)} \times 297.15\ \text{K}}{4.27\ \text{L}} \approx 0.242\ \text{atm} \)

Answer:

0.242 atm