1.4 Equilibrium Flashcards

1
Q

Define dynamic equilibrium

A

a reaction in which the rate of the forward reaction is equal to the rate of the backward reaction

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2
Q

What are the conditions for achieving dynamic equilibrium?

A

must take place in a closed system

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3
Q

Give the equation for the Haber process and state its conditions

A

N2(g) + 3H2(g) ⇌ 2NH3(g)

450ºC and 250atm

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4
Q

Give the equilibrium equation for the Haber process

A

Kc = [NH3]^2 / [N2][H2]^3

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5
Q

What is Kc?

A

The equilibrium constant

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6
Q

How are units calculated for the equilibrium constant?

A

based on the reaction’s equilibrium equation - all concentrations are mol/dm^3, but the units for Kc will vary as each reaction will have different amounts of products/reactants and different powers raised (derived from balanced stoichiometric equation)

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7
Q

What is the significance of the numerical size of the equilibrium constant?

A

The position of equilibrium - if the equilibrium constant is much greater than 1, products predominate over reactants (due to the nature of the equilibrium equation)

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8
Q

What factor affects the size of the Kc value?

A

temperature

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9
Q

What happens to Kc if the temperature increases in an endothermic reaction?

A

Kc increases - equilibrium position shifts towards products

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10
Q

What happens to Kc if the temperature decreases in an endothermic reaction?

A

Kc decreases - equilibrium position shifts towards reactants

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11
Q

What happens to Kc if the temperature increases in an exothermic reaction?

A

Kc decreases - equilibrium position shifts towards reactants

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12
Q

What happens to Kc if the temperature decreases in an exothermic reaction?

A

Kc increases - equilibrium position shifts towards products

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