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Le Châteliers Principle

Le Châtelier's Principle. “If a chemical system at equilibrium experiences a change in concentration temperature



Section 13.7 Le Chateliers Principle Workshop – Chem 201

So why do I have to know the Le Chatelier's Principle? Because it's really useful and helps to predict the effects of changes in concentration



4.0 Le Chateliers Principle 4.1 Le Chateliers Principle Le

4.1 Le Chatelier's Principle. Le Châtelier's principle states that if a system at equilibrium is subjected to an external stress the equilibrium will shift 



Green Chemistry - Equilibrium/Le Chateliers Principle

Provide students with an understanding of the concept of chemical equilibrium and to demonstrate. Le Chatelier's Principle i.e. if a stress is applied to a 



EQUILIBRIUM

In accordance with the Le Chatelier's principle the concentration stress of removed Fe3+ is relieved by dissociation of [Fe(SCN)]2+ to replenish the Fe3+ ions.



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Le Chateliers Principle

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Applications of Le-Chateliers Principle.

The Le-Chateliers principle has a great significance for the chemical (2) Applications to the physical equilibrium: Le-Chatelier's principle is ...



Section 19.1. Acid-Base Buffer Solutions

(example of Le Chatelier's Principle). = the shift in an equilibrium caused by the addition (or removal) of one of the species participating in the equilibrium.



Chapter 14. CHEMICAL EQUILIBRIUM

Le Chatelier's Principle: If a system at equilibrium is disturbed by an external stress the system adjusts to partially offset the stress as the system 

Chem 30: Equilibrium

Welter Class Notes

4.0 IH FOMPHOLHU·V 3ULQŃLSOH

4.1 IH FOMPHOLHU·V 3ULQŃLSOH

Le Châtelier's principle states that if a system at equilibrium is subjected to an external stress, the equilibrium will shift to minimize the effects of that stress.

External stresses in this situation are

factors that will change the rate of either the forward or reverse reaction.

In other words, an action that changes

the temperature, pressure, or concentration of reactants, or presence of a catalyst, in a system at equilibrium stimulates a response that counteracts said change while a new equilibrium condition is established.

4.2 Changes in Concentration

According to Le Châtelier, if we were to increase the concentration of A in the reaction below, the equilibrium position will move so that the concentration of A decreases again by reacting it with B to form more C and D. The equilibrium moves to the right. In the opposite case, in which the concentration of A is decreased, the position of equilibrium will move so that the concentration of A increases again. More C and D will react to replace the A that has been removed. The position of equilibrium moves to the left.

Chem 30: Equilibrium

Welter Class Notes

4.3 Changes in Volume & Pressure

* Changing the pressure or volume will only affect the reaction if gases are present. * Increasing the pressure (typically by reducing volume) results in the position of equilibrium moving towards the side with fewest moles of gas molecules. When pressure is decreased, the equilibrium will move to favor the side with the most moles of gas. If both sides of the equation have the same number of moles of gas, then there will be no change in the position of equilibrium.

4.4 Changes in Temperature

If the temperature is increased, then the position of equilibrium will move so that the temperature is reduced again. Thus, increasing the temperature favours the endothermic reaction. Suppose the system is in equilibrium at 300°C, and the temperature is increased 500°C. To cool down, it needs to absorb the extra heat added. In the case, the back reaction is that in which heat is absorbed. The position of equilibrium therefore moves to the left. The new equilibrium mixture contains more

A and B, and less C and D.

Chem 30: Equilibrium

Welter Class Notes

Decreasing the temperature favours the exothermic reaction, thus replacing the heat that was removed. * The main effect of temperature on equilibrium is however in changing the value of the equilibrium constant. * When temperature changes cause an equilibrium to shift, one entire side of the reaction equation is favoured over the other side. Mathematically, this will alter the value of Keq as follows: Keq = [products] [reactants] if the forward reaction is favoured more products are produced; fewer reactants Keq will increase if the reverse reaction is favoured fewer products; more reactants Keq will decrease

4.5 Addition of a Catalyst

Adding a catalyst will not affect the position of an equilibrium. A catalyst speeds up both the forward and the reverse reactions, so there is no uneven change in reaction rates. Generally, a catalyst will help a reaction to reach the point of equilibrium sooner, but it will not affect the equilibrium otherwise.

Chem 30: Equilibrium

Welter Class Notes

Examples:

1. For the reaction below, predict the direction the equilibrium will shift given the following

changes. Temperature and volume are held constant.

2 NO2 (g) + 7 H2 (g) ļ3 (g) + 4 H2O(g)

a. addition of ammonia b. removal of nitrogen dioxide c. removal of water vapour d. addition of hydrogen

2. The pressure on each of the following systems is increased by decreasing the volume of the

container. Explain whether each system would shift in the forward direction, the reverse direction, or stay the same. a. 2 SO2 (g) + O2 (g) 2 SO3 (g) b. H2 (g) + I2 (g) 2 HI(g) c. CaCO3 (s) CaO(s) + CO2 (g) d. AgCl(s) Ag1+(aq) + Cl1-(aq)

3. In each of the following equilibria, would you increase or decrease the temperature to force

the reaction in the forward direction? a. H2 (g) + CO2 (g) H2O(g) + CO(g) ǻ b. 2 SO2 (g) + O2 (g) 2 SO3 (g) ǻ-198 kJ

4. For each of the equilibria in Question 3 will the value for Keq increase or decrease if the

temperature is raised?

Chem 30: Equilibrium

Welter Class Notes

4B0 IH FOMPHOLHU·V 3ULQŃLSOH

4.1 IH FOMPHOLHU·V 3ULQŃLSOH

Le Châtelier's principle states that if a system at equilibrium is subjected to an external stress, _________________________________________________.

External stresses in this situation are

factors that will change the rate of either the forward or reverse reaction.

In other words, an action that changes

the_____________, _____________, or _____________ of reactants, or presence of a _____________ in a _____________________________ _____________________________ _____________________________.

4.2 Changes in Concentration

According to Le Châtelier, if we were to _____________ the concentration of A in the reaction below, the equilibrium position will move so that the concentration of A decreases again by reacting it with B to form more C and D. The equilibrium moves to the _____________. In the opposite case, in which the concentration of A is _____________, the position of equilibrium will move so that the concentration of A increases again. More C and D will react to replace the A that has been removed. The position of equilibrium moves to the _____________.

Chem 30: Equilibrium

Welter Class Notes

4.3 Changes in Volume & Pressure

* Changing the pressure or volume will only affect the reaction if gases are present. * _____________ the pressure (typically by reducing volume) results in the position of equilibrium moving towards the side with ___________ moles of gas molecules. When pressure is _____________, the equilibrium will move to favor the side with the _____________ moles of gas. If both sides of the equation have the _____________ number of moles of gas, then there will be _____________in the position of equilibrium.

4.4 Changes in Temperature

If the temperature is increased, then the position of equilibrium will move so that the temperature is reduced again. Thus, _____________ the temperature favours the _____________ reaction. Suppose the system is in equilibrium at 300°C, and the temperature is increased 500°C. To cool down, it needs to absorb the extra heat added. In the case, the back reaction is that in which heat is absorbed. The position of equilibrium therefore moves to the left. The new equilibrium mixture contains more

A and B, and less C and D.

Chem 30: Equilibrium

Welter Class Notes

_____________ the temperature favours the _____________ reaction, thus replacing the heat that was removed. * The main effect of temperature on equilibrium is however in changing the value of the _____________ _____________. * When temperature changes cause an equilibrium to shift, one entire side of the reaction equation is favoured over the other side. Mathematically, this will alter the value of Keq as follows: Keq = [products] [reactants] if the forward reaction is favoured more products are produced; fewer reactants Keq will increase if the reverse reaction is favoured fewer products; more reactants Keq will decrease

4.5 Addition of a Catalyst

Adding a catalyst will _____ affect the position of an equilibrium. A catalyst speeds up both the forward and the reverse reactions, so there is no uneven change in reaction rates. Generally, a catalyst will help a reaction to reach the point of equilibrium __________, but it will not affect the equilibrium otherwise.

Chem 30: Equilibrium

Welter Class Notes

Examples

1. For the reaction below, predict the direction the equilibrium will shift given the following

changes. Temperature and volume are held constant.

2 NO2 (g) + 7 H2 (g) ļ3 (g) + 4 H2O(g)

a. addition of ammonia ______________________________________________ b. removal of nitrogen dioxide ______________________________________________ c. removal of water vapour ______________________________________________ d. addition of hydrogen ______________________________________________

2. The pressure on each of the following systems is increased by decreasing the volume of the

container. Explain whether each system would shift in the forward direction, the reverse direction, or stay the same. a. 2 SO2 (g) + O2 (g) 2 SO3 (g) ______________________________________________ b. H2 (g) + I2 (g) 2 HI(g) ______________________________________________ c. CaCO3 (s) CaO(s) + CO2 (g) ______________________________________________ d. AgCl(s) Ag1+(aq) + Cl1-(aq) ______________________________________________

3. In each of the following equilibria, would you increase or decrease the temperature to force

the reaction in the forward direction? a. H2 (g) + CO2 (g) H2O(g) + CO(g) ǻ b. 2 SO2 (g) + O2 (g) 2 SO3 (g) ǻ-198 kJ

4. For each of the equilibria in Question 2 will the value for Keq increase or decrease if the

temperature is raised?

Chem 30: Equilibrium

Welter Class Notes

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