CHEM 1R03 Lecture Notes - Lecture 26: Equilibrium Constant, Electronegativity, Solubility Equilibrium

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Lecture Twenty-Six

Le Chatelier’s Principle (Continued)

•Effect of concentration: adding a reactant will decrease the amounts of the other

reactants and increase the amount of the products and form a new position of

equilibrium

•The position will shift towards the products

•Removing a reactant will increase the amounts of the other reactants and decrease

the amounts of the products —> position shifts towards the reactants

•Remember: removing a product can allow us to drive a reaction to completion

•Effect of pressure: changing the pressure of one gas is like changing its

concentration

•The same effect occurs as changing the concentration on the position of

equilibrium

•Increasing the pressure on the system causes the position of equilibrium to shift

towards the side of the reaction with the fewer gas molecules

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•Effect of volume: decreasing the volume of the system increases its pressure

•The pressure is reduced by the reduction of gas molecules

•For volume, the opposite effect happens if the system pressure is decreased

•Effect of temperature: the equilibrium constant will change if the temperature

changes

•For exothermic reactions (energy released), heating the system will decrease K

•In this situation, think of heat as a product of the reaction therefore, the position of

equilibrium shifts toward the reactant side

•For endothermic reactions (energy absorbed), heating the system will increase K

•For this, you must think of heat as a reactant so the position of equilibrium will shift

towards the products

•Cooling an exothermic or endothermic reaction will have the opposite effects on K

•Solubility products: even insoluble salts dissolve somewhat in water (insoluble =

less than 0.1 gram per 100 grams of water)

•The solubility of insoluble salts is described in terms of equilibrium between the

undissolved solid and aqueous ions is expressed as: AnXm (s) <—> n A+ (aq) + m Y

— (aq)

•The equilibrium constant is the solubility product

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Related Questions

choose:

Use LeChatelier's principle to predict the effect, if any, of removing CH₄ from the equilibrium system, described below, in a closed container. Select the single best answer.

C(s) + 2 H₂(g) â CH₄(g) + 18 kcal

	1-Equilibrium shifts right favoring products
	2-No effect
	3-Equilibrium shifts left favoring reactants

----------------

Use LeChatelier's principle to predict the effect, if any, of adding H₂ to the equilibrium system, described below, in a closed container. Select the single best answer.

C(s) + 2 H₂(g) â CH₄(g) + 18 kcal

1-No effect

2-Equilibrium shifts left favoring reactants

3-Equilibrium shifts right favoring products

-------------

Will an increase in pressure increase, decrease, or have no effect on the concentration of

NO(g)

in the following reaction? Click in the answer box to display choices.

N₂(g) + O₂(g) â 2NO(g)

	1-decrease NO(g)
	2-no effect on NO(g)
	3-increase NO(g)

----------------

Endothermic reactions are never spontaneous.

1-True

2-False

------------------

Write the equilibrium constant expression for the following reaction. Note: you can make subscripts in word by using the Ctrl and the =; superscripts are made by Ctrl, Shift, =.

N₂ + 3H₂ Ã 2NH₃

Also need help with these

State the Le Chatelierâs Principle

Change	Equilibrium shifts
Increase a reactant
decrease reactant
Increase product
decrease product

Volume changes

Change	Equilibrium shifts
Change	Reactants have more moles	Products have more moles
Increase volume
Decrease volume

The effect of temperature changes: Think of heat as a reactant (endothermic) or a product (exothermic) and use the same rules for concentration affects.

Change	Equilibrium shifts
Change	endothermic	exothermic
Add heat
Remove heat

CHEM 1R03 Lecture Notes - Lecture 26: Equilibrium Constant, Electronegativity, Solubility Equilibrium

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