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Pre AP Chemistry > Kinetics and Equilibrium > Flashcards

Kinetics and Equilibrium Flashcards

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1
Q

What is collision theory?

A

In order for collisions to occur there must be an effective collision

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2
Q

What makes an effective collision?

A
  • Sufficient (enough) energy

- Proper orientation

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3
Q

Why do reactants need sufficient Kinetic energy to cause reactions?

A

It increases the rate of the reaction and the number of collisions!

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4
Q

What are the factors that affect reaction rate?

A 
Temperature
Pressure
Concentration
Surface Area
Nature of Reactants
Catalysts
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5
Q

How does Temperature affect reaction rate?

A

-Molecules move faster causing more collisions

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6
Q

How does Concentration affect reaction rate?

A

-More molecules (high concentration) causes increased reaction rate

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7
Q

How does Surface Area affect reaction rate?

A

Having more surface area to gain sufficient energy and have more collisions

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8
Q

What does a catalyst do?

A

Increases reaction rate by lowering activation energy!

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9
Q

How does Pressure affect reaction rate?

A
  • ONLY FOR GASES!*

- Compressed particles lead to less space and more collisions

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10
Q

How do Nature of Reactants affect reaction rate?

A
  • Fastest reaction are ionic aqueous solutions

- Slowest reactions are molecular which take longer to separate

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11
Q

What is activation energy?

A

The energy needed to start a reaction

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12
Q

What is heat of reaction also called?

A

ENTHALPY

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13
Q

Exothermic:

A
  • Heat Released
  • Products LESS energy than reactants
  • Heat of reaction is NEGATIVE
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14
Q

Endothermic:

A
  • Heat absorbed
  • Products MORE energy than reactants
  • Heat of reaction is POSITIVE
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15
Q

What does a system want:

Order or Disorder?

A

Systems lean towards DISORDER and lower energy!

Called ENTROPY

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16
Q

Order of phases from highest entropy to lowest entropy:

A

G ——> L ——> S

17
Q

Which reactions are more spontaneous, Exothermic or Endothermic?

A

Exothermic reactions are more spontaneous!

18
Q

The higher the energy content, the LESS STABLE a compound

A

Endothermic reactions → Less stability

Exothermic reactions → More stability

19
Q

Negative ΔH:

A

Amount of Energy RELEASED in KJ

20
Q

Positive ΔH:

A

Amount of energy ABSORBED in KJ

21
Q

What is equilibrium?

A

When the rate of the forward reaction EQUALS the rate of the reverse reaction

22
Q

If you’re adjusting temp, conc, shifting, etc. are you in equilibrium?

A

NO!

23
Q

At Equilibrium:

A

All observable properties are CONSTANT
Amount of reactants and products are CONSTANT
Equilibrium only occurs in a CLOSED system

24
Q

What are the 3 types of Equilibrium?

A
  • Phase Equilibrium (phase changes)
  • Solution Equilibrium (w dissolved & undissolved solute)
  • Chemical Equilibrium (forward = reverse)
25
Q

Predict 2 conditions that might cause a system in equilibrium, to suddenly no longer be in equilibrium

A

-Increase temp
-Increase Concentration
-Increase Pressure
(Or decrease)

26
Q

What is Le Chatelier’s Principle?

A

If stress is added to a system at equilibrium, the equilibrium will shift in a way to RELIEVE the stress

27
Q

If a substance’s concentration is increased:

A

SHIFT AWAY from itself

28
Q

If a substance’s concentration is decreased:

A

SHIFT TOWARDS itself

29
Q

If temperature is increased:

A

Shift away from heat

30
Q

If temperature is decreased:

A

Shift towards the heat

31
Q

If pressure is increased on GASES:

A

Shift towards less moles of gas

32
Q

If pressure is decreased on GASES:

A

Shift towards more moles of gas

33
Q

What is a successful collision?

A

One that causes a reaction!

34
Q

Determining Enthalpy (Heat of Reaction)

A

H products - H reactants

Pre AP Chemistry (11 decks)

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