Consider the following chemical equilibrium of the gas phase reaction at a constant temperature: $A (g) ⇌ B (g) + C (g)$
If $p$ being the total pressure, $K_{p}$ is the pressure equilibrium constant and $α$ is the degree of dissociation, then which of the following is true at equilibrium?

Question

Consider the following chemical equilibrium of the gas phase reaction at a constant temperature:

A (g) ⇌ B (g) + C (g)

If

p

being the total pressure,

K_{p}

is the pressure equilibrium constant and

α

is the degree of dissociation, then which of the following is true at equilibrium?

Accepted Answer

Correct answer: D. (d) A (g ) ⇌B (g )+C (g ) t=0 a 0 0 t=t a (1- ) aα aα a moles of A (g ) taken initially and at time Now moles fraction of A (g ) ,B (g ) and C (g ) are X_A= a- aαa+ aα= 1- 1+ X_B= aαa+ aα= 1+ X_C= aαa+ aα= 1+ Now if P is total pressure then partial pressure of A (g ) ,B (g ) and C (g ) are P_A= ( 1- 1+ )P P_B= ( 1+ )P P_C= ( 1+ )P K_P= ( 1+ )P ( 1+ )P ( 1- 1+ )P K_P= ^2P1- ^2As K_P is only function of temperature. So as P ↑ ↓

$Consider the following chemical equilibrium of the gas phase reaction at a constant temperature: A (g) ⇌ B (g) + C (g) If p being the total pressure, K_{p} is the pressure equilibrium constant and α is the degree of dissociation, then which of the following is true at equilibrium?$

Solution

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