for the following reaction, determine which way the equilibrium would shift, toward the products or toward the reactants, given the proposed change. assume the reaction is endothermic.
To determine which way the equilibrium would shift for an endothermic reaction, we need to consider Le Chatelier’s principle. According to Le Chatelier’s principle, when a change is applied to a system at equilibrium, the system will react in such a way as to counteract the effect of the change.
In the case of an endothermic reaction, if the temperature is increased, the equilibrium will shift towards the products. This is because, by increasing the temperature, we are adding more energy to the system. To absorb this excess energy, the equilibrium will favor the endothermic reaction, which is the direction that consumes heat.
On the other hand, if the temperature is decreased, the equilibrium will shift towards the reactants. Lowering the temperature reduces the energy available in the system, so the equilibrium will favor the exothermic reaction, which releases heat.
It’s important to note that these changes in equilibrium position occur in order to maintain a constant temperature. The equilibrium position will shift in the direction that minimizes the change caused by the applied change (increase or decrease in temperature).
It’s worth mentioning that concentration changes, pressure changes (in gaseous reactions) and changes in volume (in reactions involving gases) can also affect the equilibrium position. However, since the question specifically mentions assuming an endothermic reaction, the focus is on the effect of temperature changes.