Consider the reaction : A⇔2B (⇔ stands for reversible). 1 mol of A and 2 mol of B are taken in a closed container at equilibrium. Suppose the pressure is increased, how much of B (by moles) will decompose to restore equilibrium ?
The Attempt at a Solution
Okay, i know that reaction will be in backward direction in this case if pressure is increased.
A ⇔ 2B
Eq initial 1mol , 2mol
Eq final 1+x mol , 2-2x mol (2x mol of B decomposes to form x mol of A)
equilibrium constant = 22 / 1 = 4
it will not change with pressure
So, (2-2x)2 / 1+x = 4
x is comming out to be 3.
But if i see, at eq final the remaining moles of B is 2-2*3, -4 !
How is it possible ? Please help me rectify my mistake.