CO (5.00 g)and CO₂ (5.00 g)were placed in a 750.0 mL container at 50.0 °C.The partial pressure of CO in the container was ________ atm.

Question

Quizplus · Accepted Answer

The molar mass of CO is 28.01 g/mol. Therefore, 5.00 g of CO is equivalent to $ \frac{5.00 \, \text{g}}{28.01 \, \text{g/mol}} = 0.1785 \, \text{mol} $. Using the ideal gas law $ PV = nRT $, where $ P $ is the pressure in atm, $ V $ is the volume in liters (0.750 L), $ n $ is the number of moles of gas (0.1785 mol), $ R $ is the ideal gas constant (0.0821 L·atm/(mol·K)), and $ T $ is the temperature in Kelvin (50.0 °C = 323.15 K), we can solve for $ P $. $$ P = \frac{nRT}{V} = \frac{(0.1785 \, \text{mol})(0.0821 \, \text{L·atm/(mol·K)})(323.15 \, \text{K})}{0.750 \, \text{L}} = 6.29 \, \text{atm} $$

CO (500 G)and CO2 (5

CO (500 G)and CO₂ (5