Use Le Chatelier’s Principle to predict how the addition of more SO3 gas will shift the equilibrium of this reaction:2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)Question 2Select one:a.shift right (in the forward direction) and then left (in the reverse direction)b.shift right (in the forward direction) to make more productsc.shift in equilibrium not caused by adding more SO3d.shift left (in the reverse direction) to make more reactants
Question
Use Le Chatelier’s Principle to predict how the addition of more SO3 gas will shift the equilibrium of this reaction:2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)Question 2Select one:a.shift right (in the forward direction) and then left (in the reverse direction)b.shift right (in the forward direction) to make more productsc.shift in equilibrium not caused by adding more SO3d.shift left (in the reverse direction) to make more reactants
Solution
According to Le Chatelier's Principle, if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. In this case, the addition of more SO3 gas increases the concentration of the product. To counteract this change and re-establish equilibrium, the reaction will shift to the left (in the reverse direction) to consume some of the added SO3 and produce more of the reactants, SO2 and O2.
So, the correct answer is:
d. shift left (in the reverse direction) to make more reactants
Similar Questions
Which way will the equilibrium shift, for the exothermic reaction below, if additional SO3(g) is added (and everything else is held constant)? 2SO2(g) + O2(g) Equilibrium arrow.jpg 2SO3(g) Group of answer choices To the left (more reactants) To the right (more products) It will not shift
How would the equilibrium of the reaction below be affected if the temperature increased?A.The concentrations of O2, SO2, and SO3 would increase.B.The concentrations of O2, SO2, and SO3 would decrease.C.The concentration of SO3 would increase.D.The concentrations of O2 and SO2 would increase.
How would the equilibrium change if the temperature were increased in SO2(g) + NO2(g) NO(g) + SO3(g) + heat?A.The amount of NO and SO3 would increase.B.The equilibrium constant would decrease.C.Only the reaction rate would change.D.The amount of NO2 and SO2 would increase.
Consider the equilibrium reaction represented by the equation: 2SO2(g) + O2(g) ⇌ 2SO3(g) ∆H = - 197 kJmol-1. At equilibrium, increase in the total pressure of the system brings aboutA. decrease in rate of the reaction of the systemB. decrease in temperature of the systemC. increase in temperature of SO3D. increase in concentration of SO2
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
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.