Consider the following reaction: If the system is currently at equillibrium, whi

Question

Consider the following reaction:

If the system is currently at equillibrium, which of the following are correct? (mark all that apply)

A) If you heat up the mixture, more products will be formed.

B) If you increase the volume of the container, more products will be formed.

C) If you add CO2, the equilibrium will shift to create more products.

D) If you add C(graphite), the equilibrium will shift to create more products.

E) If you add more CO, the equilibrium will shift to create more products.

ANSWERS: A, B, C, but why?

Explanation / Answer

A)

Forward reaction is endothermic 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, forward reaction will be favoured

Equilibrium moves to product side

Answer: True

B)

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 product has more gaseous molecule

So equilibrium will move to right

Equilibrium moves to product side

Answer: True

C)

we are adding a reactant

According to Le Chatelier's Principle,

Adding reactant will shift reaction towards product side

Equilibrium moves to product side

Answer: True

D)

Adding solid or liquid doesn't affect equilibrium

No effect on equilibrium

Answer: false

E)

we are adding a product

According to Le Chatelier's Principle,

Adding product will shift reaction towards reactant side

Equilibrium moves to reactant side

Answer: false

Answer: A,B,C

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