Into a 3.50-liter container at 25°C are placed 1.10 mol of O₂ gas and 4.68 mol of solid C (graphite). If the carbon and oxygen react completely to form CO(g), what will be the final pressure in the container at 25°C?

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Quizplus · Accepted Answer

Given that 1.10 mol of $O_2$ reacts with 4.68 mol of solid C (graphite) to form CO, the limiting reactant needs to be identified first. The balanced chemical equation for the reaction is:$$C + \frac{1}{2}O_2 \rightarrow CO$$From the equation, 1 mol of $C$ reacts with 0.5 mol of $O_2$ to produce 1 mol of $CO$. Therefore, 1.10 mol of $O_2$ can react with 2.20 mol of $C$ to form 2.20 mol of $CO$, since $O_2$ is the limiting reactant.The final amount of $CO$ gas formed is 2.20 mol. Using the ideal gas law $PV = nRT$, where $P$ is the pressure, $V$ is the volume (3.50 L), $n$ is the number of moles of gas (2.20 mol), $R$ is the ideal gas constant (0.0821 L·atm/mol·K), and $T$ is the temperature in Kelvin (25°C = 298 K), the final pressure can be calculated as follows:$$P = \frac{nRT}{V}$$$$P = \frac{2.20 \times 0.0821 \times 298}{3.50}$$$$P = \frac{53.8836}{3.50}$$$$P \approx 15.4 \, \text{atm}$$Therefore, the final pressure in the container is approximately 15.4 atm.

Into a 350-Liter Container at 25°C Are Placed 1