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Lecture 7

CHE 132 Lecture 7: CHE 132 Lecture 7Premium

1 pages27 viewsSpring 2019

Course Code
CHE 132
Fernando Raineri

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CHE 132 Lecture 7: Chemical Equilibrium
Gases and aqueous solutions can easily change in concentration
You should omit solids and pure liquids during reactions when calculating the K
Their reactivity doesn’t change and they will often change the result of the actual
value of K
Also omit H2O if it is a product or reactant. The concentration will not change by
a large amount so we can neglect its value
Reversing a reaction is when you go from reverse to forward or vice versa. The K
value of the reverse can be discovered by 1 / K
Remember to use stoichiometric coefficients when dealing with K. You put these
numbers in the exponents in the reaction
If you combine two reactions, it is the same as multiplying the two K values
The reaction quotient (Q) is similar to K except that you can use concentrations
at any state for Q. For K, you can only use concentrations at equilibrium
If K=Q then the reaction is at equilibrium
If Q < K then the products will be lower and you have more reactants. This will
cause the reaction to shift to the right so that you can make more products
If Q > K then the products will be greater than reactants. This will make the
reaction shift to the left causing more reactants to be made because of the
excess products
In either case, the reaction will always want to move toward equilibrium
Le Chatelier’s principle says that when a reaction is not in equilibrium anymore, it
will try to get back to equilibrium
If you add more reactant then more product will form
If you add more product then more reactants will form
If you remove a product or reactant then more product or reaction will be created
You can improve a reaction yield by adding reactants or removing a product. All
of these are valid reasons to creating more products
Increasing the pressure will increase the products when n < 0
The increase in pressure will factor the side with fewer moles of gas
Increasing temperature will add heat to the reaction
If the reaction is exothermic then heat will be a product of the reaction. Similar
can be said about endothermic in that it will be a reactant in the reaction
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