Which way will the equilibrium shift, for the endothermic reaction below, if additional N2O4(g) is added (and everything else is held constant)?N2O4(g) 2NO2(g)Group of answer choicesTo the left (more reactants)To the right (more products)It will not shift
Question
Which way will the equilibrium shift, for the endothermic reaction below, if additional N2O4(g) is added (and everything else is held constant)?N2O4(g) 2NO2(g)Group of answer choicesTo the left (more reactants)To the right (more products)It will not shift
Solution
The equilibrium of a reaction can be shifted by changing the concentrations of the reactants or products. This is known as Le Chatelier's Principle.
In the given reaction, N2O4(g) is a reactant. If we add more N2O4(g), we are increasing the concentration of the reactant. According to Le Chatelier's Principle, the equilibrium will shift to counteract this change.
In this case, the equilibrium will shift to the right (more products) to reduce the concentration of the added reactant (N2O4(g)). This is because the reaction will try to consume the added N2O4(g) by producing more NO2(g).
So, the answer is: To the right (more products).
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