The moles of N₂O₄ and NO₂ at equilibrium are 1 and 2 respectively total pressure at equilibrium is 9 atm. Kp for the reaction is 12.
The reaction is given as :
N₂O₄(g) ⇄ 2NO₂(g)
the total pressure , P = 9 atm
the Kp expression is as :
Kp = ( PNO₂ )² / (PN₂O₄)
the Daltons law of partial pressure is given as :
PNO₂ = XNO₂ P total
XNO₂ = mole fraction of NO₂
PNO₂ = ( 2 / 1+2) 9
= 6 atm
PN₂O₄ = (1 / 3) × 9 = 3 atm
therefore equilibrium constant Kp is given as :
Kp = 6² / 3
Kp = 12
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