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** $$PV = nRT$$ $$P = \frac{nRT}{V}$$ **Step 4: Substitute values** Using $R = 0.0821 \text{ L·atm/(mol·K)}$: $$P = \frac{(1.136 \times 10^{-3})(0.0821)(303)}{4.6}$$ $$P = \frac{0.0283}{4.6} = 0.00615 \text{ atm}$$ Converting to other units if needed: - **In mmHg:** $0.00615 \times 760 = 4.7 \text{ mmHg}$ - **In kPa:** $0.00615 \times 101.325 = 0.62 \text{ kPa}$ **Answer: Approximately 0.0062 atm or 4.7 mmHg** (Option D depends on the given choices)