Question

For the reaction N2(g)+O2(g)⇌2NO(g) classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction. Drag the appropriate items to their respective bins.

Answer 1

The question is incomplete, complete question is;

For the reaction:

$N_2(g)+O_2(g)\rightarrow 2NO(g)$

classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction.

a) half oxygen

b) double oxygen

c) double nitrogen

d) half nitrogen

e) double nitrogen monoxide

f) half nitrogen monoxide

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.

On an addition of product

• If we add more product at an equilibrium, the equilibrium will move in backward direction towards the reactant side and vice versa.
• If we add more reactant at an equilibrium, the equilibrium will move in forward direction towards the product side and vice versa.

a) Half oxygen

Here reactant is reducing, which means that concentration of product is increasing at equilibrium. So, to in order to counter the change the equilibrium will move backward that is leftward direction .

b) Double oxygen

Here reactant is increasing , which means that concentration of product is deceasing at equilibrium. So, to in order to counter the change the equilibrium will move forward that is rightward direction.

c) Double nitrogen

Here reactant is increasing , which means that concentration of product is decreasing at equilibrium. So, to in order to counter the change the equilibrium will move forward that is rightward direction.

d) Half nitrogen

Here reactant is reducing, which means that concentration of product is increasing at equilibrium. So, to in order to counter the change the equilibrium will move backward that is leftward direction .

e) Double nitrogen monoxide

Here product is increasing , which means that concentration of reactant is decreasing at equilibrium. So, in order to counter the change the equilibrium will move backward that is leftward direction.

f) Half nitrogen monoxide

Here product is decreasing , which means that concentration of reactant is increasing at equilibrium. So, in order to counter the change the equilibrium will move forward that is rightward direction.