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Question

For the decomposition reaction4HNO3(g)4NO2(g)+2H2O+O2(g) if we start with only the reactant HNO3 and p = equilibrium pressure, the equilibrium constant Kp is:


A

Kp = x7P7x4

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B

Kp = 1024x7(P4x)4

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C

Kp = 7x(p7x)

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D

Kp = (P7x)7(P7x)4

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Solution

The correct option is B

Kp = 1024x7(P4x)4


Let the initial pressure be P. For constant T and volume, equal moles of all ideal gases contribute equal partial pressures.

4HNO3(g)4NO2(g)+2H2O+O2

4HNO3 4NO2 2H2O O2
t=0 P 0 0 0
At equilibrium P4x 4x 2x x


Total pressure at equilibrium = sum of all partial pressures = p = P + 3x

Kp=[4x]4[2x]2x[P4x]4=1024x7(P4x)4

This kind of playing around with partial pressures is convenient when only either reactants or products are present initially. Otherwise we have to take existing individual partial pressures into account as well.


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