Chapter 14-Chemical Equilibrum Flashcards
What does it mean when K>1
- products are favoured
- reaction lies to the right
What does it mean when K<1?
- reactants are favoured
- reaction lies to the left
What does it mean when K=1
- neither reaction is favoured
- forward reaction proceeds about halfway to completion
Q
- reaction proceeds to the right
- products need to be formed
what doeQ>K mean?
- reaction proceeds to the left
- reactants need to be formed
Q=K
-reaction is at equilibrum
Increasing the amount of reactant (Q
-causes a shift to the right
Decreasing the amount of reactant (Q>K)
-causes a shift to the left
Increasing the amount of product (Q>K)
- causes a shift to the right
Decreasing the amount of product (Q
-causes a shift to the right
Decrease in volume, increase in pressure
- shift to the side with fewer moles
Increase in volume, decrease in pressure
- shift to the side with more moles
Increasing the temperature of an exothermic reaction
- reaction shifts left
- decreases K
Decreasing the temperature of an exothermic reaction
- reaction shifts right
- increase K
increasing temp of an endothermic reaction
- reaction shifts left
- increases K
decreasing temp of an endothermic reaction
- shift left
- decreases K
Five Strong Acids
HCI, HBR, HI, HNO3, HClO4, H2SO4
Five Strong Bases
Li, Na, K, Ca, Ba, Sr
How to find pH of strong acid?
- no ICE Table jsut plug it into pH equation
How to find pH of a strong base?
-no need for ICE Table, just plut into poH= -log(OH)
How to find pH of a weak acid?
- ICE Table
how to find pH of weak base?
- ICE Table, use Kb
how to find pH of one strong+one weak acid?
- take the H30+ of the strong acid
how to find pH of two weak acids?
- take the H30+ of the acid with the higher ka, only applicable if Ka differs by 100x
