Into a 2.22-liter container at 25°C are placed 1.23 moles of O₂gas and 3.20 moles 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

The balanced chemical equation is:C + O₂ → COThe number of moles of CO produced is equal to the number of moles of O₂, which is 1.23 moles. The total number of moles of gas in the container is therefore 1.23 moles + 3.20 moles = 4.43 moles. The final pressure in the container can be calculated using the ideal gas law:PV = nRTwhere 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.Substituting the given values into the ideal gas law, we get:P(2.22 L) = (4.43 moles)(0.0821 Latm/(molK))(298 K)Solving for P, we get:P = 27.1 atmTherefore, the final pressure in the container is 27.1 atm.

Into a 222-Liter Container at 25°C Are Placed 1