General Chemistry Ch 6. Equilibrium Flashcards

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1
Q

Reversible reactions

A

Steady state in which energy is minimized in entropy is maximized, dynamic

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2
Q

Dynamic

A

Reactions are still occurring, just at a constant rate

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3
Q

Law of mass action

A

Gives the expression for the equilibrium constant, Keq

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4
Q

Chemical equilibria

A

Dynamic, concentrations of reactants and products remain constant because the rate of the forward reaction equals the rate of the reverse reaction

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5
Q

Law of mass action

A

Gives the expression for the equilibrium constant Keq, if a system is at equilibrium at a constant temperature, then…

Key = [C]^c*[D]^d/[A]^a/[B]^b

Does not include pure solids and liquids, only gases and aqueous species

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6
Q

Reaction quotient

A

Q - Same form as keq but can be calculated at any concentrations at any given time during a reaction, relates the reactant and product concentrations at any given time during a reaction

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7
Q

Equilibrium constant

A

Keq - ratio of products to reactants at equilibrium with each species raised to its stoichiometric coefficients, constant at a constant temperature

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8
Q

Q

A

DeltaG<0 and the reaction proceeds in the forward direction

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9
Q

Q=Keq

A

DeltaG=0 and the reaction is in dynamic equilibrium

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10
Q

Q>Keq

A

DeltaG>0 and the reaction proceeds in the reverse direction

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11
Q

Keq>1

A

The products are present in greater concentrations at equilibrium

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12
Q

Keq=1

A

Products and reactants are both present at equilibrium at reasonably similar levels

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13
Q

Keq<1

A

The reactants are present in greater concentration at equilibrium

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14
Q

Keq«<1

A

The amount of reactants that have been converted to products can be considered negligible in comparison to the initial concentration of reactants

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15
Q

Le Chateliers principle

A

States that when a chemical system experiences a stress, it will react so as to restore equilibrium

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16
Q

Types of stresses applied to a system

A

Changes in concentration, pressure and volume, and temperature

17
Q

Changing concentration Le Chateliers

A

Increasing the concentration of reactants or decreasing the concentration of products will shift the reaction to the right, increasing the concentration of products or decreasing the concentration of reactants will shift the reaction to the left

18
Q

Changing pressure/volume Le Chateliers

A

Increasing pressure on a gaseous system (decreasing volume) will shift the reaction toward the side with fewer moles of gas, decreasing pressure (increasing volume) will shift the reaction toward the side with more moles of gas

19
Q

Changing temperature Le Chateliers

A

Increasing the temperature of an endothermic reaction or decreasing the temperature of a exothermic reaction will shift the reaction to the right, decreasing the temperature of an endothermic reaction or increasing the temperature of an exothermic reaction will shift the reaction to the left

20
Q

Kinetic products

A

Higher in free energy than thermodynamic products and can form at lower temperature, sometimes termed “fast” products because they can form more quickly under such conditions

21
Q

Thermodynamic products

A

Lower in free energy than kinetic products and are therefore more stable, despite proceeding more slowly than the kinetic pathway, the thermodynamic pathway is more spontaneous (more negative deltaG)