N2O4(g) ↔ 2NO2(g) In the endothermic reaction above, more product formation will be favoured by
Question 1 Report
N2O4(g) ↔ 2NO2(g)
In the endothermic reaction above, more product formation will be favoured by
Answer Details
In the endothermic reaction N2O4(g) ↔ 2NO2(g), more product formation will be favored by a decrease in pressure. This is because the reaction produces two moles of gas for every one mole of N2O4 that reacts. According to Le Chatelier's Principle, when the pressure on a system is decreased, the equilibrium will shift to the side of the reaction with more moles of gas to compensate for the decrease in pressure. In this case, the equilibrium will shift to the side of the reaction that produces more gas molecules, which is the side with more NO2(g) molecules. Therefore, a decrease in pressure will favor the formation of more NO2(g) molecules, resulting in more product formation.
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