equilibrium - Kc and Kp Flashcards

1
Q

equation for Kc

A

Kc = [products] / [reactants]

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2
Q

what is homogenous equilibria

A
  • species all have the same state
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3
Q

what is heterogenous equilibria

A
  • species with different states

- only include gases/aq in the Kc expression

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4
Q

mole fraction equation

A

x(A) = number of moles of A / total moles in gas mixture

sum of MF = 1

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5
Q

partial pressure equation

A

p(A) = x(A) x total pressure in system

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6
Q

Kp expression

A

Kp = p(products) / p(reactants)

- only include gases

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7
Q

magnitude of K relate to eq position

A
K = 1 : eq halfway between R + P
K = greater than 1 : towards P
K = less than 1 : towards R
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8
Q

effect of temp on Kp

A

Exothermic:

  • temp inc
  • Kp decreases
  • eq shifts to left

Endothermic

  • temp inc
  • Kp inc
  • eq shifts to the right
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9
Q

effect of conc + pressure on K

A
  • no effect
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10
Q

catalyst effect on k

A
  • no effect
  • catalysts affect rate of a reaction
  • not the position of equilibrium
  • speed up forward and reverse reaction by the same factor
  • so equilibrium is reached quicker.
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