If the partial pressure of a gas is increased, and everything else stays the same, then the total pressure is increased and your statements above are correct; i.e., increased P and the equilibrium shifts to the side with fewer mols of gas.
P vs T follows Charles' Law.
What's the difference between the pressure of a system and the partial pressures in relation to Le Chatelier's principles?
I know that when the pressure of the system is increased, it goes to the side with less moles/particles and when decreased it will go to the side with the most.
But I was wondering what about partial pressures? Are they similar to concentrations in the way that if you increase the partial pressure of a substance, the equilibrium will move to the side where that substance isn't located?
What happens to the pressure of the system and the partial pressures for changes such as temperature, concentrations, volume, etc.?
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