A 5.00 L flask contains 3.50 g of sulfur trioxide, 2.45 g of carbon monoxide, and 3.99 g of argon all at 35°C. What is the pressure (in atm) in the flask?

Question

Quizplus · Accepted Answer

To find the total pressure in the flask, we can use the ideal gas law, $PV = nRT$, where $P$ is the pressure, $V$ is the volume, $n$ is the number of moles, $R$ is the ideal gas constant, and $T$ is the temperature in Kelvin. First, we convert the temperature to Kelvin: $35°C + 273.15 = 308.15 K$. Next, we calculate the moles of each gas:- For sulfur trioxide ($SO_3$), the molar mass is $32.06 (S) + 3 \times 16.00 (O) = 80.06 g/mol$. Moles of $SO_3 = \frac{3.50 g}{80.06 g/mol} = 0.0437 mol$.- For carbon monoxide ($CO$), the molar mass is $12.01 (C) + 16.00 (O) = 28.01 g/mol$. Moles of $CO = \frac{2.45 g}{28.01 g/mol} = 0.0875 mol$.- For argon ($Ar$), the molar mass is $39.95 g/mol$. Moles of $Ar = \frac{3.99 g}{39.95 g/mol} = 0.0999 mol$.Total moles = $0.0437 mol + 0.0875 mol + 0.0999 mol = 0.2311 mol$.Using the ideal gas law, $P = \frac{nRT}{V}$, where $R = 0.0821 L \cdot atm/(mol \cdot K)$, $V = 5.00 L$, and $T = 308.15 K$, we find:$$P = \frac{0.2311 mol \times 0.0821 L \cdot atm/(mol \cdot K) \times 308.15 K}{5.00 L} = 1.17 atm.$$

A 500 L Flask Contains 3