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UK - Che 107 - Class Notes - Week 5

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Exam 2 MaterialWe also discuss several other topics like What are examples of nonprogrammed decisions?

Chapter 13: Chemical Kinetics

- Skip “ measuring reaction rates” 13.2

Chemical Kinetics is the study of the speeds (rates) at which chemical reactions occurDon't forget about the age old question of What does apical meristem mean?

Speed = ==If you want to learn more check out csu awm

Reaction rate = =

- Reaction rates change with time [M/s] → molarity per second

- Average rate = rate over a period of time

- instantaneous rate = the rate at any point in time

- Based on slope of the curve at that point
- Draw a tangent to the curve at the point of interest

- Reaction rate equation: aA + bB → cC + dD
- = - = + = +

**Cannot predict the rate at a future time using this!!We also discuss several other topics like What does GDP stand for?

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Example: H2O2 can be used as a disinfectant; it decomposes as : 2H2O2 → 2H2O2?

Rate = + = + We also discuss several other topics like Enumerate the models of interpersonal communication.

(x) = 0.0022 M / s

= 0.0044 M / s

Rate law: the relationship between the rate of reaction and concentration of reactants

Rate constant(k): a constant of proportionality in the rate law

For the reaction: aA - dD

The rate law is: rate = k[A]h n is determined experimentally

Rate equation: rate law:

= - = k[A]h

Chapter 13

Rate = K[A]h

N = 0 zero order

- Rate is independent of concentration

H = 1 first order

- Rate is proportional to concentration

N = 2 second order

- Rate is proportional to concentration squared

K = rate constant

N = order of reaction

Rate = initial rate

A = concentration

If the concentration doubles, the rate doesn’t change

- 1rst order kinetics = if the concentration doubles, the rate doubles
- 2nd order kinetics = if the concentration doubles, the rate quadruples
- When you have multiple reactants, compare that where only one reactant changes concentration
- The overall order of the reaction is the sum of orders of the reactants

Rate Law:

- The relationship between the rate of the reaction and the concentration of reactants

Integrated rate law:

- relationship between concentration and time

Zero order integrated rate law:

[A]t = kt + [A]0

Y = mx + b

Y = Concentration of A at time t

Kt = rate constant

0 = concentration of A at time t = 0

First order integrated rate law

In [A]t = -kt + in [A]0

Second order integrated rate law

= kt +

Example: the gas phase decomposition of NO2 to NO and O2 is a second order reaction with k = 0.543 M-1S-1. If the initial concentration of NO2 in a closed vessel is 0.0500M, what is the remaining concentration after 0.500h?

2nd order = = kt + 0.500h x x = 1800s

= = 0.543 x 1800s +

= 997 - 4 1/ M

1/ 997.4 1/M

= 1.00x 10-3M