Questions: Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system? SO2(g) + NO2(g) = SO3(g) + NO(g) The reaction will shift in the direction of products. The reaction will shift to decrease the pressure. No change will occur since SO3 is not included in the equilibrium expression. The reaction will shift in the direction of reactants. The equilibrium constant will decrease.

Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system?
SO2(g) + NO2(g) = SO3(g) + NO(g)
The reaction will shift in the direction of products.
The reaction will shift to decrease the pressure.
No change will occur since SO3 is not included in the equilibrium expression.
The reaction will shift in the direction of reactants.
The equilibrium constant will decrease.

Transcript text: Consider the following reaction at equilibrium. What effect will adding more SO 3 have on the system? \[ \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g})=\mathrm{SO}_{3}(\mathrm{~g})+\mathrm{NO}(\mathrm{~g}) \] The reaction will shift in the direction of products. The reaction will shift to decrease the pressure. No change will occur since $\mathrm{SO}_{3}$ is not included in the equilibrium expression. The reaction will shift in the direction of reactants. The equilibrium constant will decrease.

Solution

Solution Steps

Step 1: Understanding the Reaction and Le Chatelier's Principle

The given reaction is at equilibrium:

\[ \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{NO}(\mathrm{~g}) \]

According to Le Chatelier's Principle, if a system at equilibrium is disturbed, the system will adjust itself to counteract the disturbance and restore a new equilibrium.

Step 2: Analyzing the Effect of Adding More SO$_3$

Adding more $\mathrm{SO}_{3}$ will increase the concentration of one of the products. According to Le Chatelier's Principle, the system will shift to counteract this change by favoring the reverse reaction, which consumes $\mathrm{SO}_{3}$ and produces $\mathrm{SO}_{2}$ and $\mathrm{NO}_{2}$.

Step 3: Determining the Direction of the Shift

Since the system will shift to reduce the concentration of $\mathrm{SO}_{3}$, it will favor the reverse reaction, shifting the equilibrium towards the reactants.