Lecture 3: Chemical Equilibrium Flashcards

1
Q

There are three requirements for a chemical reaction to occur

A
  1. Molecules must collide
  2. Molecules must be in the proper orientation when they collide
  3. Molecules must have the appropriate amount of energy during collision
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2
Q

is the minimum amount of energy particles must possess for collisions to result to the occurrence of a chemical reaction

A

ACTIVATION ENERGY

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3
Q

is how fast products are formed in a certain amount of time measured in amount of time

A

Reaction rate

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4
Q

Factors affecting the rate of chemical reactions

A
  1. Temperature
  2. Reactant Concentration
  3. Catalyst
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5
Q

Increasing the temperature in a reaction increases the kinetic energy of particles

A

TEMPERATURE

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6
Q

More reactant molecules will increase the number of collisions leading to the occurrence of chemical reactions

A

REACTANT CONCENTRATION

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7
Q

Lowers the activation energy of a chemical reactions making it easier for products to form from reactants

A

CATALYST

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8
Q

When we substitute the values of the molar concentrations, we get the equilibrium constant which is a ______________

A

unitless numerical value

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9
Q

Large Kc

A

favors products

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10
Q

Small Kc

A

favors reactants

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11
Q

The state of equilibrium of a reversible chemical reaction can be disrupted by external factors

A

LE CHATELIER’S PRINCIPLE

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12
Q

SHIFT: Decreasing the volume

A

Fewer moles of gas

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13
Q

SHIFT: Increasing the volume

A

More moles of gas

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14
Q

ENDO SHIFT: Increasing the temperature

A

Products (forward reaction)

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15
Q

ENDO SHIFT: Decreasing the temperature

A

Reactants (reverse reaction)

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16
Q

EXO SHIFT: Increasing the temperature

A

Reactants (reverse reaction)

17
Q

EXO SHIFT: Decreasing the temperature

A

Products (forward reaction)

18
Q

SHIFT CATALYST: Increasing the rates equally

A

No effect