Video: EC17-18-S1-Q12

Calculate the value of Kp in the reaction shown, given the following partial pressures: P(N₂) = 0.4 atm, P(O₂) = 2 atm, and P(NO₂) = 4 atm. N₂(g) + 2O₂(g) is in equilibrium with 2NO₂(g)

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Video Transcript

Calculate the value of Kp in the reaction shown, given the following partial pressures: P(N₂) equal to 0.4 atmospheres, P(O₂) equal to two atmospheres, and P(NO₂) equal to four atmospheres.

N₂ gas plus 2O₂ gas is in equilibrium with 2NO₂ gas. Kp is the equilibrium constant. Kp is defined as the product of the partial pressures of the products raised to their stoichiometric coefficients divided by the same for the reactants. This is equal to the partial pressure of nitrogen dioxide squared divided by the partial pressure of nitrogen multiplied by the partial pressure of oxygen squared. This is equal to four squared divided by 0.4 multiplied by two squared. This is equal to 10. So this is what you would need to write, and here is our answer.

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