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When the below reaction occurs at 55°C, the respective pressures of N2O4 (g) and NO2 (g) at2.equilibrium are 0.212 atm and 0.254 atm. Calculate both equilibrium constants, Kp and KçN2O4 (g)2 NO2 (g)

Question
When the below reaction occurs at 55°C, the respective pressures of N2O4 (g) and NO2 (g) at
2.
equilibrium are 0.212 atm and 0.254 atm. Calculate both equilibrium constants, Kp and Kç
N2O4 (g)
2 NO2 (g)
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When the below reaction occurs at 55°C, the respective pressures of N2O4 (g) and NO2 (g) at 2. equilibrium are 0.212 atm and 0.254 atm. Calculate both equilibrium constants, Kp and Kç N2O4 (g) 2 NO2 (g)

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Step 1

A reversible chemical reaction can move in either forward or backward direction. The stage of a reversible reaction at which the rate of forward and backward reaction become equal to each other is called an equilibrium stage.

 

Step 2

The equilibrium constant for a reaction is the ratio of equilibrium concentration of product and reactant. If the reaction is given in gaseous state, then the equilibrium pressure must be considered.

Step 3

The Kp expression for the below ...

N2042) 2NO,
'2(g)
'4(g)
2
NO2(8)
[PNO
К.
р
[P
N204()
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N2042) 2NO, '2(g) '4(g) 2 NO2(8) [PNO К. р [P N204()

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Equilibrium Concepts

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