# Chem202 Chap 14 & 15

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1. Average reaction rate for
A----->B
• rate=-^A/^t
• rate=^B/^t
• ^ is delta
2. Stoichiometry and Reaction Rate
aA+bB---->cC+dD
• rate=-1/a(^[A]/^t)
• rate=-1/b(^[B]/^t)
• rate=1/c(^[C]/^t)
• rate=1/d(^[D]/^t)
3. rate law
aA+bB---->cC+dD
rate=k[A]x[B]y
4. reation order and units of k
0====M/s
1====1/s
2====1/Ms
3====1/M2s
5. 1st order half life
t1/2=.693/k
half life of a first order reaction is independent of the initial concentration of the reactant.
6. 2nd order half life
t1/2=1/k[A]o
half life is inversely proportional to initial reactant concentration.
7. 0 order half life
t1/2=[A]o/2k
?
8. collision theory
• the reaction rate is directly proportional to the number of molecular collisions per second.
• ratea=number of collisions/s
9. activation energy Ea
minimum amount of energy required to initiate a chemical reaction.
10. activated complex or transition state.
when molecules collide in an effective collision. highest amount of potential energy.
11. unimolecular elementary reaction
• one reactant molecules
• A------>products
12. bimolecular elementary reaction
• two reactant molecules
• A+A---->products
• A+2B---->products
13. termolecular elementary reaction
• three reactant molecules
• A+B+C--->products
14. reaction order for each reactant in an elementary reaction is equal to its stoichiometric coefficient in the chemical equation for that step.
• A+A---->products
• 2A------>products
• rate=k[A]2
15. catalyst
is a substance that increases the rate of a chemical reaction without itself being consumed.
16. heterogeneoues catalyst
the reactant and the catalyst are in different phases. The catalyst is usually a solid and the reactants are either gases or liquids
17. homogenous catalyst
the reactants and the catalyst are dispersed in a single phase usually liquid
18. Reversible process
A chemical reaction in which the products can also be consumed to produce reactants, a process known as the revers reaction
19. Equilibrium
the condition where the forward and reverse reactions are occurring at the same rate and there is no net change in the reactant and products concentrations over time
20. Reaction Quotient (Qc)
Qc=[C]c[D]d/[A]a[B]b
(also Kc at equilibrium)
is the product of the product concentrations over the product of the reactant concentrations with each concentration raised to a power equal to the corresponding stoichiometric coefficients in the balanced chemical equation. Law of Mass Action
21. Equation reversed = 1/Kc1
Equation mulitplied by 2 =(Kc1)2
Two equations added = Kc1*Kc2
22. Kp=Kc(RT)^n
Delta n=number of moles of product-number of moles of reactant
23. Kc=prod/react
raised to the power of the coefficient in front
24. if Qc<Kc ---Reactant to products
if Qc>Kc ---Products to reactants
• +prod shift left
• -prod shitf right
• +react shift right
• -react shift left
25. + pressure-----shift equil to side w/ fewest moles
+volume-----shift equil to side w/ most moles
26. temp is the only factor that changes the equilibrium constant
catalyst shifts neither the equilibrium or equilibrium constant
 Author: Jamess0688 ID: 69393 Card Set: Chem202 Chap 14 & 15 Updated: 2011-02-28 03:04:11 Tags: Chemical kinetics Chemical Equilibrium Folders: Description: for exam 2 Show Answers: