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If more reactants are added (increasing the number of moles), the reaction will "shift right" meaning more products will be formed to offset that change. Now that there are more reactants available, more products must form to keep the reaction in equilibrium. If reactants are removed (decreasing the number of moles), the reaction will "shift left" meaning less products will be formed. You can use similar logic to explain what happens when the number of moles on the products side increases or decreases. Hope that helps!
Usually when we determine a shift in a reaction by comparing the number of moles on each side of the reaction it is usually when analyzing a change in the reaction given a change in pressure. In such a case, if you increase pressure, a reaction would shift to the side with less moles of gas in order to offset the increase in pressure by reducing the amount of molecules in the defined volume. The opposite situation would also have similar logic. It is important to note that when there is a change in pressure, it really only affects the reaction if there is a corresponding affect on volume, as that relates to changes in concentration.
Hope that helps!
Hope that helps!
There is a natural point where there will the energy will be the lowest for a certain reaction. Some reactions will be at their lowest energy when there are a relatively high number of products, and vice versa. Thus, when there is a change in the number of moles of a reaction, then that reaction will shift to ensure that it is once again at the ratio of products to reactants that is the most stable.
When the pressure is increased by decreasing volume, the reaction will move in whichever direction will reduce the pressure. This means that it will move towards the side with fewer moles (so fewer molecules), which causes the pressure to decrease.
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