Question

If the reaction below is at equilibrium, which of the following will shift the equilibrium to the right?

                        2 CO(g) + O₂(g) <-> 2 CO₂(g)   ΔH is negative

A) increasing the amount of CO₂ in the vessel            

B) increasing the temperature

C) increasing the volume of the container   

D) adding a catalyst

E) none of these

Answer 1

Lets see the effect of A

we are adding a product

According to Le Chatelier's Principle,

Adding product will shift reaction towards reactant side

Answer: Equilibrium moves to reactant side

Lets see the effect of B

Forward reaction is exothermic in nature

we are increasing temperature or adding heat here

so, according to Le Chatelier's principle,

equilibrium will move in direction which absorbs heat

hence, backward reaction will be favoured

Answer: Equilibrium moves to reactant side

Lets see the effect of C

We are increasing volume here

In other words we are trying to decrease pressure

so, according to Le Chatelier's principle,

Reaction will try to increase the pressure

Hence it will move in a direction which have more gaseous molecules

Here reactant has more gaseous molecule

So equilibrium will move to left

Answer: Equilibrium moves to reactant side

Lets see the effect of D

Catalyst doesn't affect equilibrium

Answer: No effect on equilibrium

we can see that none of them moves the reaction to product side

Answer: E