Question

Kc for the reaction
A(g) +B(g) =2C(g) is 3.0 at 400 K. In an experiment 'a' mol of A is mixed
with 3 mol of B in a 1-L vessel. At equilibrium 3 mol of C is formed. The value
of 'a' will be
(a) 4.5 mol (b) 9.5 mol (C) 2.5 mol (d) 3.5 mol (e) 7 mol​

Answer 1

Explanation:

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Answer 2

Given info : Kc for the reaction A(g) +B(g) = 2C(g) , is 3.0 at 400 K.

In an experiment 'a' mol of A is mixed with 3 mol of B in a 1-L vessel. At equilibrium 3 mol of C is formed.

To find : the value of a

solution : here,

A + B ⇒ 2C

at t = 0 a 3 0

at eql a - x 3 - x 2x

but given 2x = 3 ⇒x = 3/2

now equilibrium constant, Kc = [C]²/[A][B]

⇒3 = (2x)²/(a - x)(3 - x)

⇒3 = 9/(a - 3/2)(3 - 3/2)

⇒1 = 3/(a - 3/2)(3/2)

⇒a - 3/2 = 2

⇒a = 2 + 1.5 = 3.5

Therefore the value of a is 3.5 mol.

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