Question
Asked Feb 29, 2020
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A sample of pure NO2 is heated to 338 ∘C at which temperature it partially dissociates according to the equation
2NO2(g)⇌2NO(g)+O2(g)
At equilibrium the density of the gas mixture is 0.525 g/L at 0.755 atm. Calculate Kc for the reaction

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Expert Answer

Step 1

The density of gas mixture = 0.525 g/L

The pressure is 0.755 atm

The dissociation of pure NO2 is,

2NO2(g)⇌2NO(g)+O2(g)

The equilibrium constant for the reaction is,

Chemistry homework question answer, step 1, image 1

The ideal gas equation at equilibrium is,

PV=nRT

The temperature is 611K.

The value of R=0.0821 L.atm/K.mol

On substituting the values in ideal gas equation,

Chemistry homework question answer, step 1, image 2

 

Step 2

The ice table for the equation (1) is given below.

Chemistry homework question answer, step 2, image 1

The total mass of mixture at equilibrium is calculated by the expression,

Chemistry homework question answer, step 2, image 2

...

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