How will an increase in pressure influence the amount of SO2(g) present at equilibrium?explain.
To determine how an increase in pressure will influence the amount of SO2(g) present at equilibrium, we need to understand Le Chatelier's principle, which states that when a system at equilibrium experiences a change in conditions, it will shift to minimize the effect of that change and establish a new equilibrium.
In this case, we're dealing with a gaseous equilibrium expressed as:
SO2(g) ⇌ SO2(g)
Let's say the forward reaction represents the formation of SO2 and the reverse reaction represents the decomposition of SO2. An increase in pressure can be achieved by decreasing the volume, increasing the concentration (if the reaction occurs in a closed container), or adding an inert gas.
When the pressure is increased, the system will shift in the direction that reduces the overall pressure. According to Le Chatelier's principle, an increase in pressure will favor the side with fewer gaseous moles. In this case, the gaseous equation has the same number of moles on both sides, so pressure has no direct effect on the equilibrium position.
Therefore, an increase in pressure will not influence the amount of SO2(g) present at equilibrium in this particular case.