Unit 4: Equilibrium and chemical systems

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graphing, math, and mixture of unit 3 rates of reaction

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<p><strong>Conditions for an equilibrium system</strong></p>

Conditions for an equilibrium system

  • a closed system (energy ONLY leaves or enters NOT MATTER)

  • reversible reaction (both forward and reverse direction)

  • reactants and products are present at the same time (rates of the forward and reverse reactions must be equal)

  • equations use this symbol “⇌

  • Solubility Equilibrium—> balance b/tw solid and ions

  • Phase Equilibrium—> balance b/tw 2 states of a substance

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<p><strong>Analyzing graphs</strong></p>

Analyzing graphs

  • on the graph, there is a constant period (reached Chemical Equilibrium)

  • the constant period is shown by the straight line/Plateau (concentration of react. and prod. will NOT CHANGE)

  • reactants never COMPLETELY “disappear”

  • Position of Equilibrium—> on the graph, it is the point where the formation of react. or prod. is favored (concentration is higher than the other)

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<p><strong>Equilibrium Law and constant</strong></p>

Equilibrium Law and constant

  • uses stoichiometric coefficients= exponents

  • “K”—> defines the equilibrium law (CONSTANT and NO UNITS)

  • K is constant UNLESS temp. change

  • Heterogenous Equilibrium—> react. and prod. are present in 2 differ states (NOT INCLUDED in the EXPRESSION for the system)

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<p><strong>‘K” in more depth</strong></p>

‘K” in more depth

  • K<1—> more react. are present

  • K=1—> 50/50

  • K>1—> more prod. are present

  • Kforward and Kreverse are INVERSLY related