At 100 °C, the reaction 2NO2(g) N2O4(g) has KP = 15.39. Suppose a mixture of these gases was prepared at 100 °C in a 400 mL vessel with the following partial pressures: Upper P Subscript UpperWord N O Sub Subscript 2 Baseline ⁢ equals 0.348 ⁢ atm and Upper P Subscript Upper N Sub Subscript 2 Subscript Upper O Sub Subscript 4 Baseline ⁢ equals 0.678 ⁢ atm. What will the partial pressures of the gases be at equilibrium? What will the total pressure of the gas mixture be? What is the total mass of gas in the reaction vessel?

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At 100 °C, the reaction 2NO2(g) N2O4(g) has KP = 15.39. Suppose a mixture of these gases was prepared at 100 °C in a 400 mL vessel with the following partial pressures: Upper P Subscript UpperWord N O Sub Subscript 2 Baseline ⁢ equals 0.348 ⁢ atm and Upper P Subscript Upper N Sub Subscript 2 Subscript Upper O Sub Subscript 4 Baseline ⁢ equals 0.678 ⁢ atm. What will the partial pressures of the gases be at equilibrium? What will the total pressure of the gas mixture be? What is the total mass of gas in the reaction vessel?

Chemistry
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PNO2 =? PN2O4 =?

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