A sealed 2.00 L container at 20.0^oC holds 150.0 g of ammonia (NH₃), 150.0 g of carbon dioxide (CO₂), and 150.0 g of nitrogen(N₂). What is the total pressure in atmospheres?

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To find the total pressure in the container, we use the ideal gas law, $PV = nRT$, where $P$ is the pressure, $V$ is the volume, $n$ is the number of moles of gas, $R$ is the ideal gas constant, and $T$ is the temperature in Kelvin. First, we convert the temperature to Kelvin: $20.0^\circ C = 293 K$. Next, we calculate the moles of each gas:- For ammonia ($NH_3$), the molar mass is $14.01 + 3(1.01) = 17.04 \, g/mol$. Moles of $NH_3 = \frac{150.0 \, g}{17.04 \, g/mol} = 8.80 \, mol$.- For carbon dioxide ($CO_2$), the molar mass is $12.01 + 2(16.00) = 44.01 \, g/mol$. Moles of $CO_2 = \frac{150.0 \, g}{44.01 \, g/mol} = 3.41 \, mol$.- For nitrogen ($N_2$), the molar mass is $2(14.01) = 28.02 \, g/mol$. Moles of $N_2 = \frac{150.0 \, g}{28.02 \, g/mol} = 5.35 \, mol$.Total moles of gas = $8.80 + 3.41 + 5.35 = 17.56 \, mol$.Using the ideal gas law, $P = \frac{nRT}{V}$, where $R = 0.0821 \, L \cdot atm/(mol \cdot K)$, $V = 2.00 \, L$, and $T = 293 \, K$:$$P = \frac{17.56 \, mol \times 0.0821 \, L \cdot atm/(mol \cdot K) \times 293 \, K}{2.00 \, L} = 211 \, atm.$$

A Sealed 2