Consider the following equilibrium system involving SO2, Cl2, and SO2Cl2 (sulfur

ID: 1008892 • Letter: C

Question

Consider the following equilibrium system involving SO2, Cl2, and SO2Cl2 (sulfuryl dichloride):

SO2(g) + Cl2(g) SO2Cl2(g)

Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case.

(a) Cl2 gas is added to the system.

1.The equilibrium will not change.

2.The equilibrium position will shift to favor the reverse reaction. (More reactants form.)

3.The equilibrium position will shift to favor the forward reaction. (More products form.)

(b) SO2Cl2 is removed from the system.

1.The equilibrium will not change.

2.The equilibrium position will shift to favor the reverse reaction. (More reactants form.)

3.The equilibrium position will shift to favor the forward reaction. (More products form.)

1.The equilibrium will not change.

2.The equilibrium position will shift to favor the reverse reaction. (More reactants form.)

3.The equilibrium position will shift to favor the forward reaction. (More products form.)

Which number matches up with the letters? Can you please explain why too?

Thank you!

SO2(g) + Cl2(g) SO2Cl2(g)

according lechatliers principle " a system at equilibrium undergoes stress.the equilibrium shifts in such a way that ,

in order to un do the stress"

a) 3.The equilibrium position will shift to favor the forward reaction. (More products form.)

b) 3.The equilibrium position will shift to favor the forward reaction. (More products form.)

c) 2.The equilibrium position will shift to favor the reverse reaction. (More reactants form.)

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