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## Homework Statement

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 ?

## Homework Equations

## 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 = 2

^{2}/ 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.