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22 Cards in this Set

  • Front
  • Back

Increase in [A]

↓[B]


↑[C] equilibrium shift --->


↑[D]

Decrease in [A]

↑[B]


↓[C] equilibrium shift <---


↓[D]

Increase in [B]

↓[A]


↑[C] equilibrium shift --->


↑[D]

Decrease in [B]

↑[A]


↓[C] equilibrium shift <---


↓[D]

Increase in [C]

↑[A]


↑[B] equilibrium shift --->


↓[D]

Decrease in [C]

↓[A]


↓[B] equilibrium shift <---


↑[D]

Increase in [D]

↑[A]


↑[B] equilibrium shift --->


↓[C]

Decrease in [D]

↓[A]


↓[B] equilibrium shift <---


↑[C]

Increase temperature


Exothermic (ΔH is negative)

↑[A]


↑[B] equilibrium shift <---


↓[C]


↓[D]

Decrease temperature


Exothermic (ΔH is negative)

↓[A]


↓[B] equilibrium shift --->


↑[C]


↑[D]

Increase temperature


Endothermic (ΔH is positive)

↓[A]


↓[B] equilibrium shift --->


↑[C]


↑[D]

Decrease temperature


Endothermic (ΔH is positive)

↑[A]


↑[B] equilibrium shift <---


↓[C]


↓[D]

Pressure conditions:

-at least one reactant or product is a gas


-the number of gaseous molecules are not equal on each side of the equation

Pressure:


Increase in Volume (of container)

Decrease in Pressure

Pressure:


Decrease in Volume (of container)

Increase in Pressure

n =

m/M

c =

n/V

pH =

-log [H⁺]

[H⁺] =

10⁻ᵖᴴ

H20(l)

H⁺ + OH⁻

H20 + H20

H3O⁺ + OH

Kw =

[H][OH⁻] = 1.00 x 10⁻¹⁴


[H3O][OH⁻] = 1.00 x 10⁻¹⁴