equilibrium I Flashcards

1
Q

where can dynamic equilibrium only happen?

A

in a closed system

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2
Q

what is the equilibrium constant?

A

Kc

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3
Q

what is the equilibrium constant for?

A

gives an idea of how far to the left or right equilibrium is

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4
Q

what is and what happens when a reaction is at equilibrium?

A

-rate of the forward reaction is equal to the rate of the backward reaction
-concentrations of reactants and products remain constant

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5
Q

how does equilibrium happen?

A

as the reactants get used up, the forward reaction slows down and as more product is formed

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6
Q

do catalysts affect the equilibrium constant?

A

-no ∴ you don’t include catalysts in expressions for equilibrium constant
-they don’t effect equilibrium concentrations of products or reactants they just speed up the rate at which dynamic equilibrium is reached

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7
Q

what type of substance is used ONLY in Kc expressions?

A

gases

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8
Q

what is heterogeneous system?

A

not all products and reactants are in the same physical state

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9
Q

what is a homogeneous system?

A

all products and reactants are in the same physical state

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10
Q

what does le chateliers principle predict?

A

what will happen if conditions are changed

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11
Q

how is equilibrium affected if you increase the concentration of a reactant?

A

equilibrium is shifted to the right

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12
Q

how is equilibrium affected if you increase the concentration of a product?

A

equilibrium is shifted to the left because equilibrium tries to remove the extra product

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13
Q

how is equilibrium affected if you increase the pressure?

A

shifts equilibrium to side with fewer gas molecules to reduce the added pressure

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14
Q

how is equilibrium affected if you decrease the pressure?

A

shifts equilibrium to side with more gas molecules to raise pressure again

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15
Q

how is equilibrium affected if you decrease the temperature?

A

shifts in the exothermic direction to try replace heat

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16
Q

how is equilibrium affected if you increase the temperature?

A

shifts in the endothermic direction to try absorb heat

17
Q

formula for partial pressure of a gas?

A

mole fraction x total pressure

18
Q

what is the mole fraction of a gas?

A

the proportion of gas in a mixture

19
Q

formula for mole fraction of gas in a mixture?

A

number of moles of gas/total number of moles of gas in the mixture

20
Q
A