Chemistry: 1.10 Equilibrium Constant, Kp
Explore how reversible reactions reach equilibrium, what conditions are required, and how the equilibrium constant reflects the position of the reaction.
what does the rate of forward reaction equal
rate of reverse reaction
Key Terms
what does the rate of forward reaction equal
rate of reverse reaction
what remains the same unless conditions are changed
concentration of reactants and products
what does Kc equal
[PRODS]/[REACTANTS]
what does the Kc indicate
the extent of the reaction- how far equilibrium lies to right/left
Kc<1
equilibrium lies to left
Kc=1
equilibrium is in the middle
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| Term | Definition |
|---|---|
what does the rate of forward reaction equal | rate of reverse reaction |
what remains the same unless conditions are changed | concentration of reactants and products |
what does Kc equal | [PRODS]/[REACTANTS] |
what does the Kc indicate | the extent of the reaction- how far equilibrium lies to right/left |
Kc<1 | equilibrium lies to left |
Kc=1 | equilibrium is in the middle |
Kc>1 | equilibrium lies to the right |
le chateliers principle | if a system in equilibrium is subjected to a change, the position of equilibrium will move in the direction which opposes that change |
what value do all reactions at equilibrium have | a kc valu |
what is a kc value based on | concentrations of all reactants and products |
kp | equilibrium constant that only involve pressure exerted by the gas molecules |
what do kp expressions only contain | the gases present in the equilibrium mixture |
what is the only factor that affects the value of an equilibrium constant | temperature |
if the temperature change caused equilibrium to shift right, what will happen to kp |
|
what will happen to kp if the temperature change causes equilibrium to shift left | decrease |
what is the partial pressure of a gas in a gas mixture | the contribution that gas makes toward the total pressure |
what is the partial pressure of each gas proportional to | its mole fraction |
partial pressure= | mole fraction of gas x total pressure |
mole fraction of a gas = | moles of that gas in mixture/total number of moles of gas in mixture |