For the following equilibrium 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen to the concentrations of each gas if the pressure is increased?SO2 and O2 will decrease; SO3 will increaseSO2, O2 and SO3 will all decreaseSO2, O2 and SO3 will all increaseSO2 and O2 will increase; SO3 will decrease
Question
For the following equilibrium 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen to the concentrations of each gas if the pressure is increased?SO2 and O2 will decrease; SO3 will increaseSO2, O2 and SO3 will all decreaseSO2, O2 and SO3 will all increaseSO2 and O2 will increase; SO3 will decrease
Solution
The equilibrium reaction is 2SO2(g) + O2(g) ⇌ 2SO3(g). This reaction is governed by Le Chatelier's Principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
In this case, if the pressure is increased, the system will try to reduce the pressure. It can do this by favoring the side of the reaction with fewer gas molecules.
Looking at the balanced equation, there are 3 gas molecules on the left (2SO2 + O2) and 2 gas molecules on the right (2SO3). Therefore, to decrease the pressure, the reaction will shift to the right, towards the side with fewer gas molecules.
So, the concentrations of SO2 and O2 will decrease (as they are being used up to form more SO3), and the concentration of SO3 will increase.
Therefore, the correct answer is "SO2 and O2 will decrease; SO3 will increase".
Similar Questions
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