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The pressure is only important for gases. An increased pressure would favor the side with fewer moles of gases. Whereas temperature affects the equilibrium constant K. I don't know why yet, but he will teach us in the later weeks.
The only thing that will change the equilibrium constant, k, is temperature. However when you increase the pressure by decreasing the volume, the concentration increases and the reaction will thus proceed to the left or right in order to return to equilibrium.
The only thing that will change K is a change in temperature. As for pressure, it does change the concentration, but it changes it proportionally so that K is still the same when you divide the products and reactants. The moles of products and reactants may change with a change in pressure, but the K should calculate out to be the same.
The only change to a system that will change the value of K is temperature. Pressure is really changing the number of mols by changing the volume. Therefore, depending on how the mols change, the equilibrium will shift to get back to that constant K. Temperature does not change the number of mols of reactants or products and therefore needs to be approached differently.
Hi! Temperature and pressure are both physical parameters that can shift the direction of the reaction to get back to equilibrium; however, changing the pressure of the reaction does not change K, but changing the temperature can change K. In terms of pressure, only compressing the system by making the volume smaller (affecting the concentrations) will shift the reaction, but adding inert gas into the system will not. Hope this helps! :)
Temperature will change the K value. For example, if a reaction is endothermic and you heat up the reaction, the forward reaction will be favored and more products will be produced. When looking at how to solve the equilibrium constant (K). More product on the numerator will mean a larger K value. Pressure on the other hand will not change the K value.
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