Question

Consider the reaction cl2(g) + i2(g) <=> 2 icl(g), which is endothermic as written. what would be the effect on the equilibrium position of removing cl2(g)? 1. reaction would go to the left, making more "reactants" 2. no change on the equilibrium position 3. reaction would go to the right, making more "reactants" 4. reaction would go to the left, making more "products" 5. reaction would go to the right, making more "products"

Answer 1

The given equilibrium reaction is,

$Cl_{2}(g)+I_{2}(g)+Heat2ICl(g)$

According to Le Chatelier's principle states that when a system in equilibrium is disturbed by varying conditions like concentration, pressure, and temperature of the system, the system tries to counter act the affect by shifting the equilibrium towards the required side.

When $Cl_{2}$ is removed from the system, the concentration of chlorine ($Cl_{2}$) decreases, the equilibrium is disturbed. So, the system tries to re-establish the equilibrium by moving in that direction which produces more of chlorine, that is towards the reactant side.

The correct answer would be: 1. reaction would go to the left, making more "reactants"