Consider the following reversible system at temperature ' T ' Kelvin: A ( g ) + 2 B ( g ) ⇌ A B 2 ( g ) ; K c = 4 1 The above equilibrium is established in a 1.0 L flask, and at eq

Question

Consider the following reversible system at temperature ' $T$ ' Kelvin:

$A_{(g)} + 2 B_{(g)} ⇌ A B_{2 (g)}$ ; $K_{c} = \frac{1}{4}$

The above equilibrium is established in a $1.0 L$ flask, and at equilibrium, $2$ moles of each A and B are present. If at $T K$ the volume is doubled and $2$ moles of B are added further, how many moles of AB₂ should be added along with 'B' so that the moles of A do not change at the new equilibrium state?

TestHub · Accepted Answer

K C ​ = [ A ] [ B ] 2 [ A B 2 ​ ] ​ ⇒ 4 1 ​ = 2 × ( 2 ) 2 x ​ ⇒ 4 1 ​ = 2 × 4 x ​ ⇒ x = 2 [ A B 2 ​ ] = 2 M . Now, let y moles of AB₂ be added. ∵ K C ​ = 2 ( 2 + 2 ) 2 ( 2 + y ) ​ ( 2 1 ​ ) − 2 = 4 1 ​ ⇒ 2 × ( 4 ) 2 ( 2 + y ) ​ × ( 2 ) 2 = 4 1 ​ y = 0

Chemistry - Chemical Equilibrium Question with Solution | TestHub

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