Question

Assume equilibrium has been reached in the following reaction:
$A\left(g\right)+B\left(g\right)\rightleftharpoons C\left(g\right)+D\left(g\right)$
On an increase in the pressure, the system will:

• A. Shift to the products
• B. Shift to the reactants
• C. Not change because pressure never affects equilibrium positions
• D. Not change because there are equal number of moles of gas in reactant and product
  

Answer 1

The correct option is D Not change because there are equal number of moles of gas in reactant and product

The given reaction is :-

$A\left(g\right)+B\left(g\right)\rightleftharpoons C\left(g\right)+D\left(g\right)$

In this reaction, the no. of moles of gaseous species are same on reactants and product side. So, As per Le Chatelier's principle, pressure will have on effect on it.