Dry ice is solid carbon dioxide. A 0.050 g sample of dry ice is placed in an evacuated 4.6 L vessel — States of Matter and Gaseous State Chemistry Question
Question
Dry ice is solid carbon dioxide. A 0.050 g sample of dry ice is placed in an evacuated 4.6 L vessel at 30ºC. Calculate the pressure inside the vessel after all the dry ice has been converted to $CO_2$ gas.
💡 Solution & Explanation
# Solution: Pressure from Sublimed Dry Ice **Step 1: Convert mass of $CO_2$ to moles** Molar mass of $CO_2$ = 12 + 2(16) = 44 g/mol $$n = \frac{0.050 \text{ g}}{44 \text{ g/mol}} = 1.136 \times 10^{-3} \text{ mol}$$ **Step 2: Convert temperature to Kelvin** $$T = 30°C + 273 = 303 \text{ K}$$ **Step 3: Apply ideal gas law** $$PV = nRT$$ $$P = \frac{nRT}{V} = \frac{(1.136 \times 10^{-3} \text{ mol})(0.0821 \text{ L·atm/mol·K})(303 \text{ K})}{4.6 \text{ L}}$$ **Step 4: Calculate** $$P = \frac{0.0284}{4.6} = 0.0062 \text{ atm} = 6.2 \times 10^{-3} \text{ atm}$$ Converting to other units: - **In mmHg:** $0.0062 \times 760 = 4.7$ mmHg - **In Pa:** $0.0062 \times 101,325 = 628$ Pa ≈ 6.3 × 10² Pa The answer is **D** (most likely 0.0062 atm or equivalent pressure in alternative units).