Calculating concenteration at equilibrium

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SUMMARY

The discussion focuses on calculating the concentration of NO2 at equilibrium for the reaction N2O4(g) ⇌ 2NO2(g) with a given equilibrium constant Kp of 0.14. The initial amount of N2O4 is 0.1 moles, and the conversion of Kp to Kc yields Kc = 0.00572. The participants highlight the necessity of knowing the volume (V) to derive a numerical answer, suggesting the use of the ideal gas equation PV = nRT to find the volume.

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  • Basic algebra for solving equations
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harambe
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Homework Statement


0.1mole of N2O4 (g) was sealed In a tube under one atmospheric conditions at 25°C.Calculate the number of moles of NO2(g) present if the equilibrium N204(g) --->2NO2(g) (Kp=0.14) is reached after some time

Homework Equations


K=[NO2]^2/[N2O4]
3. The attempt at the solution

N204(g) --->2NO2(g)

O. 1 0
O. 1-x x

Converting Kp into Kc gives me Kc=0.00572

Kc[NO2]^2/[N2O4]V where V is the volume

But I don't know the volume so I am not able to calculate here.. . Any hint on how to solve this
 
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Yes I think you can't get a numerical answer if you don't know V.

So just get a general answer with an expression that contains v.
 
harambe said:
But I don't know the volume so I am not able to calculate here.. . Any hint on how to solve this

Couldn't you find volume from the ideal gas equation: PV = nRT ?
 

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