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3 years ago

What change would shift the equilibrium system to the left?

Chemistry

2 answers:

ArbitrLikvidat [17]3 years ago

5 0

Answer: The correct option is, Adding more of gas C to the system.

Explanation :

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation :

$A(g)+B(s)+Energy\leftrightharpoons 3C(g)$

This is a type of Endothermic reaction because heat is absorbed in the reaction.

For the given options :

Option A: Adding more of gas C to the system

If the concentration of gas C that is the product is increased, so according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease of concentration takes place. Therefore, the equilibrium will shift in the left direction.

Option B: Heating the system

If the temperature is increased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where increase in temperature occurs. As, this is an endothermic reaction, forward reaction will decrease the temperature. Hence, the equilibrium will shift in the right direction.

Option C: Increase the volume

If the volume of the container is increased, the pressure will decrease according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where increase in pressure is taking place. As the number of moles of gas molecules is greater at the product side. So, the equilibrium will shift in the right direction.

Option D: Removing some of gas C from the system

If the concentration of gas C that is the product is decreased, so according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease of concentration takes place. Therefore, the equilibrium will shift in the right direction.

Hence, the correct option is, Adding more of gas C to the system.

SVEN [57.7K]3 years ago

3 0

Answer:

Adding more of gas C to the system

Explanation:

Le Châtelier's principle states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.

1) Adding more of gas C to the system:

Adding more C gas will increase the concentration of the products side. So, the reaction will be shifted to the left to attain the equilibrium again.

2) Heating the system:

Heating the system will increase the concentration of the reactants side as the reaction is endothermic. so, the reaction will be shifted to the right to attain the equilibrium again.

3) Increasing the volume:

has no effect since the no. of moles of gases is the same in both reactants and products sides.

4) Removing some of gas C from the system:

Removing some of gas C from the system will decrease the concentration of the products side. So, the reaction will be shifted to the right to attain the equilibrium again.

So, the right choice is: Adding more of gas C to the system.

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