Chapter 14 Flashcards

1
Q

Equilibrium is a state in which

A

there are no observable changes as time goes by.

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2
Q

chemical equilibrium is achieved when:

A
  • the rates of the forward and reverse reactions are equal and
  • the concentrations of the reactants and products remain constant
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3
Q

homogenous equilibrium applies to reactions in which

A

all reacting species are in the same phase.

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4
Q

eterogenous equilibrium applies to reactions in which

A

reactants and products are in different phases.

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5
Q

The concentration of _____ and ________ are not included in the expression for the equilibrium constant.

A

solids and pure liquids

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6
Q

If a reaction can be expressed as the sum of two or more reactions, the equilibrium constant for the overall reaction is given by

A

the product of the equilibrium constants of the individual reactions.

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7
Q

Writing Equilibrium Constant Expressions

A
  1. The concentrations of the reacting species in the condensed phase are expressed in M. In the gaseous phase, the concentrations can be expressed in M or in atm.
  2. The concentrations of pure solids, pure liquids and solvents do not appear in the equilibrium constant expressions.
  3. The equilibrium constant is a dimensionless quantity.
  4. In quoting a value for the equilibrium constant, you must specify the balanced equation and the temperature.
  5. If a reaction can be expressed as a sum of two or more reactions, the equilibrium constant for the overall reaction is given by the product of the equilibrium constants of the individual reactions.
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8
Q

The reaction quotient (Qc)is calculated by

A

substituting the initial concentrations of the reactants and products into the equilibrium constant (Kc) expression

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9
Q

IF

A
  • Qc > Kcsystem proceeds from right to left to reach equilibrium
  • Qc = Kc the system is at equilibrium
  • Qc < Kcsystem proceeds from left to right to reach equilibrium
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10
Q

Calculating Equilibrium Concentrations

A
  1. Express the equilibrium concentrations of all species in terms of the initial concentrations and a single unknown x, which represents the change in concentration.
  2. Write the equilibrium constant expression in terms of the equilibrium concentrations. Knowing the value of the equilibrium constant, solve for x.
  3. Having solved for x, calculate the equilibrium concentrations of all species.
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11
Q

Le Châtelier’s Principle

A

If an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is partially offset as the system reaches a new equilibrium position.

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12
Q

.•Adding a Catalyst

A
  • does not change K
  • does not shift the position of an equilibrium system
  • system will reach equilibrium sooner
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13
Q

Catalyst lowers Ea for

A

both forward and reverse reactions.Catalyst does not change equilibrium constant or shift equilibrium.

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