Regents level kinetics and equilibrium review
1. all reactions need collisions to take place, the more frequent the collisions the
faster the reactions and the less time needed
2. Increased temperature, increased concentration(molarity), increased surface
area(powder), and a catalyst all make reactions faster
3. Catalyst provide an alternate pathway with lower activation energy
4. physical and chemical systems may go to equilibrium in a closed system
5. saturated solutions are at equilibrium, rate of dissolving = rate of crystallization
6. freezing point, boiling point, closed bottle with water in it all have equilibrium
7. RECC Rates Equal Concentrations Constant
8. increasing a reactant concentration shifts a system to the right which increases
product and decreases the reactants – you can’t make product without consuming
reactant
9. decreasing a concentration shifts to the same side you decreased from
10. adding heat favors the endothermic process – remember ice melts better with
more heat
11. increasing pressure will shift to the side with less moles of gas, if moles of gas are
not different pressure has no effect
12. a catalyst does not cause a shift, it only make the system reach equilibrium faster
K > 1 products are favored
K< 1 reactants are favored
K = [products]x
[Reactants] y
each is raised to the power of the coefficients
Solids and liquids are left out