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I like to think of it as a balancing act. If you decrease the volume on one side which increases the pressure, the reaction will favor the side with less molecules because the pressure needs to go somewhere else, if that makes sense.
If you increase the pressure of the reaction, the reaction will shift to the side with fewer moles of gas. If you decrease the pressure of the reaction, the reaction will shift to the side with the greater number of moles of gas. A change in pressure causes a shift in the reaction because it alters the concentrations of the substances in the reaction, which causes it to no longer be at K.
Increasing the pressure will shift the reaction to the side with fewer moles of gas and decreasing the pressure will shift the reaction to the side with more moles of gas. If there is an equal number of moles on the reactants and products, then there will be no change.
If the pressure is increased the reaction would want to go back to equilibrium, so the reaction will shift to the side with fewer gas particles. If the pressure were to decrease then the reaction would go towards the side with more gas particles.
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