Karteikarten
Equilibrium Constant - Part II
Karten in diesem Stapel (14)
- 1Kc/ Equilibrium constantA measure of the position of the equilibrium; the magnitude of an equilibrium constant indicates whether there are more reactants or more products an equilibrium system.
- 2Homogeneous EquilibriumAn equilibrium in which all the species are making up the reactants and products have the same physical state.
- 3Heterogeneous EquilibriumAn equilibrium in which the species making up the reactants and products have different physical states.
- 4EquilibriumThe rate of the forwards reaction is equal to the reverse.
- 5KpUsed for gaseous equilibria. It doesn't use concentrations, instead requires partial pressures.
- 6Partial PressureIt is the contribution each gas makes towards the total pressure. = mole fraction x total pressure.
- 7What doesn't affect K?Concentration, pressure and catalysts don't affect K as they are quantities.
- 8What affects K?Temperature does as its a condition.
- 9Exothermic (increasing temperature)Favours endothermic direction
Shifts to the left
Kp decreases - 10Exothermic (decreasing temperature)Favours exothermic direction
Shifts to the right
Kp increases - 11Endothermic (increasing temperature)Favours the endothermic direction
Shifts to the right
Kp increases - 12Endothermic (decreasing temperature)Favours the exothermic direction
Shifts to the left
Kp decreases - 13Changing [B] / [A]Disables the equilibrium because K is a constant value and the expression is now higher/lower than k. [B] or [A] must increase or decrease until the expression is equal to k. When they are equal to k, equilibrium is restored.
- 14Temperature (K)Quantities [B] / [A] don't change. Equilibrium is affected by temperature. K must change to a new value. This will disable the equilibrium as the values don't match k. So the quantities must adjust.
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- Der Nutzer hat seine Fachbereichs-Information gelöscht. Karteikarten am Equilibrium Constant - Part II, erstellt von Gelöschter Nutzer am 23/09/2017.
- Erstellt von
- Gelöschter Nutzer · Sep 2017
- Aktualisiert
- 23 Sep 2017
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- 22
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- Erstellt von Chloe Drewery · 10 Sep 2017
- Kopiert von Chloe Drewery · 23 Sep 2017
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