# Ch. 14, Chemical Kinetics

### 19 terms by am_kinnear

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### What is the equation for rate reactions?

[(∆)Something changing]/[Change in(∆) time]

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### What is the equation for rate laws?

rate=k[reactant]^m[reactant]^n; k is determined experimentally

2/1

### What is the equation for solving for k?

K= rate/([react]^m[react]^n)

### What is the equation for First-Order Reactions

rate= -∆[X]/∆t(←time) = k[X]^1

### What is the equation for Second-Order Reactions

rate= -∆[X]/∆t(←time) = k[X]^2

### What is the equation for Zero-Order Reactions

rate= k[react]^0 = k; [react] = -kt + [react]˅0

rate= k[X]^3

### What two things need to be present for reactions to occur?

Collisions, Collisions with proper orientation

### Define activation energy

Minimum energy required for collisions to be productive

### When a bond is breaking, is it endo or exo, and is energy being given to or taken from the surroundings?

Endo, energy is given off to surroundings

### When a bond is forming, is it endo or exo, and is energy being given to or taken from the surroundings?

Exo, energy taken from surroundings

### On the reaction pathway, name the normal steps (A-E &Ea)

Step A = reactants, Step B = Activated complex, Ea, Step C = intermediate (more stable than B & D), Step D = activated complex, Ea, Step E = Products, Step Ea = Reverse, D, C, etc..

Temperature

### Why does k increase with increasing temperatures?(4 reasons)

1. Greater avg velocity & greater avg KE, 2. Increases in frequency of collisions, 3. Increase in number of collisions with proper orientation, 4. Increases number of collisions with sufficient energy

### What is the Arrhenius equation?

k = Ae^(-Ea/RT); ln(k) = (-Ea/R)(1/T) + ln(A)

### What does A mean in the Arrhenius equation

A is the frequency factor; frequency of collisions, fraction of collisions with proper orientation

Example: