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.

Double(nitogen monoxide)

halve (nitrogen monoxide)

double(nitrogen)

halve(oxygen)

double(oxygen)

halve(nitrogen)

Question 2) For the reaction C(s)+H2O(g)<--- --->H2(g)+CO(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.

remove some water,

add some hydrogen,

remove some solid carbon,

remove some hydrogen,

remove some carbon monoxide,

add some solid carbon

add some carbon monoxide,

add some water.

Answer 1

Concepts and reason

If the concentration of the reactants or products in a chemical reaction at equilibrium is changed, then the position of equilibrium shifts in the opposite direction so as to counteract the change.

Fundamentals

According to Le-Chatelier’s principle, when a reaction is in dynamic equilibrium and its equilibrium is disrupted by changing temperature, pressure, concentration or volume, then the equilibrium position of the reaction shifts by acting against the introduced effect.

(1a)

Consider the following reaction:

When the concentration of nitrogen monoxide is doubled, then the position of equilibrium moves to the left so that the concentration of nitrogen monoxide decreases again.

(1b)

Consider the following reaction:

When the concentration of nitrogen monoxide is halved, then the position of equilibrium moves to the right so that the concentration of nitrogen monoxide increases again.

(1c)

Consider the following reaction:

When the concentration of nitrogen is doubled, then the position of equilibrium moves to the right so that the concentration of nitrogen decreases again.

(1d)

Consider the following reaction:

When the concentration of oxygen is halved, then the position of equilibrium moves to the left so that the concentration of oxygen increases again.

(1e)

Consider the following reaction:

When the concentration of oxygen is doubled, then the position of equilibrium moves to the right so that the concentration of oxygen decreases again.

(1f)

Consider the following reaction:

When the concentration of nitrogen is halved, then the position of equilibrium moves to the left so that the concentration of nitrogen increases again.

(2a)

Consider the following reaction:

When the concentration of water is decreased by removing some amount of it, then the position of equilibrium moves to the left so that the concentration of water increases again.

(2b)

Consider the following reaction:

When the concentration of hydrogen is increased by adding some amount of it, then the position of equilibrium moves to the left so that the concentration of hydrogen decreases again.

(2c)

Consider the following reaction:

When some amount of solid carbon is removed from the reaction, then there is no shift in the position of equilibrium as the concentration of pure solid carbon is fixed. However, the concentration of pure gases is subject to change because of their tendency to compress easily.

(2d)

Consider the following reaction:

When the concentration of hydrogen is decreased by removing some amount of it, then the position of equilibrium moves to the right so that the concentration of hydrogen increases again.

(2e)

Consider the following reaction:

When the concentration of carbon monoxide is decreased by removing some amount of it, then the position of equilibrium moves to the right so that the concentration of carbon monoxide increases again.

(2f)

Consider the following reaction:

When some amount of solid carbon is added, then there is no shift in the position of equilibrium as the concentration of pure solid carbon is fixed. However, the concentration of pure gases is subject to change because of their tendency to compress easily.

(2g)

Consider the following reaction:

When the concentration of carbon monoxide is increased by adding some amount of it, then the position of equilibrium moves to the left so that the concentration of carbon monoxide decreases again.

(2h)

Consider the following reaction:

When the concentration of water is increased by adding some amount of it, then the position of equilibrium moves to the right so that the concentration of water decreases again.

Ans: Part 1a

[Answer]
‎

When the concentration of nitrogen monoxide is doubled, then there will be a leftward shift in the direction of the reaction to counteract this change such that the concentration of nitrogen monoxide decreases again according to Le-Chatelier’s principle.

Part 1b

[Answer]
‎

When the concentration of nitrogen monoxide is halved, then there will be a rightward shift in the direction of the reaction to counteract this change such that the concentration of nitrogen monoxide increases again according to Le-Chatelier’s principle.

Part 1c

[Answer]
‎

When the concentration of nitrogen is doubled, then there will be a rightward shift in the direction of the reaction to counteract this change such that the concentration of nitrogen decreases again according to Le-Chatelier’s principle.

Part 1d

[Answer]
‎

When the concentration of oxygen is halved, then there will be a leftward shift in the direction of the reaction to counteract this change such that the concentration of oxygen increases again according to Le-Chatelier’s principle.

Part 1e

[Answer]
‎

When the concentration of oxygen is doubled, then there will be a rightward shift in the direction of the reaction to counteract this change such that the concentration of oxygen decreases again according to Le-Chatelier’s principle.

Part 1f

[Answer]
‎

When the concentration of nitrogen is halved, then there will be a leftward shift in the direction of the reaction to counteract this change such that the concentration of nitrogen increases again according to Le-Chatelier’s principle.

Part 2a

[Answer]
‎

When some water is removed, then there will be a leftward shift in the direction of the reaction to counteract this change such that the concentration of water increases again according to Le-Chatelier’s principle.

Part 2b

[Answer]
‎

When some hydrogen is added, then there will be a leftward shift in the direction of the reaction to counteract this change such that the concentration of hydrogen decreases again according to Le-Chatelier’s principle.

Part 2c

[Answer]
‎

When some solid carbon is removed, then there will be no shift in the direction of the reaction because its concentration is fixed.

Part 2d

[Answer]
‎

When some hydrogen is removed, then there will be a rightward shift in the direction of the reaction to counteract this change such that the concentration of hydrogen increases again according to Le-Chatelier’s principle.

Part 2e

[Answer]
‎

When some carbon monoxide is removed, then there will be a rightward shift in the direction of the reaction to counteract this change such that the concentration of carbon monoxide increases again according to Le-Chatelier’s principle.

Part 2f

[Answer]
‎

When some solid carbon is added, then there will be no shift in the direction of the reaction because its concentration is fixed.

Part 2g

[Answer]
‎

When some carbon monoxide is added, then there will be a leftward shift in the direction of the reaction to counteract this change such that the concentration of carbon monoxide decreases again according to Le-Chatelier’s principle.

Part 2h

[Answer]
‎

When some water is added, then there will be a rightward shift in the direction of the reaction to counteract this change such that the concentration of water decreases again according to Le-Chatelier’s principle.