Solid carbon dioxide is placed into a Ziploc bag. Solid carbon dioxide sublimes (turns directly from a solid to a gas) at a rate of 0.726 g/minute. If the pressure builds to 3.75 atm at a temperature of 21.1^oC, what is the final volume of the bag after 4.97 minutes? (Assume the volume of the solid carbon dioxide is negligible.) A) 37.9 mL B) 0.379 mL C) 1.98 mL D) 0.528 mL E) 528 mL

Question

Quizplus · Accepted Answer

First, calculate the total mass of CO2 that sublimes: $0.726 \, \text{g/minute} \times 4.97 \, \text{minutes} = 3.61 \, \text{g}$.Next, use the ideal gas law $PV = nRT$, where $P = 3.75 \, \text{atm}$, $R = 0.0821 \, \text{L atm/mol K}$, and $T = 21.1^\circ C + 273.15 = 294.25 \, K$. Convert the mass of CO2 to moles: $n = \frac{3.61 \, \text{g}}{44.01 \, \text{g/mol}} = 0.082 \, \text{mol}$.Solve for $V$: $V = \frac{nRT}{P} = \frac{(0.082 \, \text{mol})(0.0821 \, \text{L atm/mol K})(294.25 \, K)}{3.75 \, \text{atm}} = 0.528 \, \text{L} = 528 \, \text{mL}$.

Solid Carbon Dioxide Is Placed into a Ziploc Bag