Use the following reaction scenario to answer the following questions
SO2(g)+Cℓ2(g)⇌SO2Cℓ2(g)ΔrH°<0SO_2 (g) + Cℓ_2 (g) ⇌ SO_2Cℓ_2 (g) \qquad Δ_rH° < 0SO2(g)+Cℓ2(g)⇌SO2Cℓ2(g)ΔrH°<0
You have prepared a container with these compounds and allowed it to come to equilibrium. You now have a choice of different ways to modify your system at equilibrium:
Assume that during each of these changes, all other parameters remain constant.
Which of these alterations would result in a decrease in the amount (in moles) of SO2Cℓ2 (g) at equilibrium?
adding a non-reactive gas, N2
removing Cℓ2 (g) from the system
adding Cℓ2 (g) to the system
increasing the temperature of the system
increasing the volume of the reaction vessel
Which of these alterations would affect the equilibrium constant, KC, for this reaction?
Which of these alterations would cause an immediate increase in the reaction quotient, QC, for this reaction?
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Le Chatelier's Principle: Equilibrium constant
Consider the following reaction:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
The measured equilibrium constant is 5.0 × 10–4 at 373 K and 0.20 at 473 K. Which of the following statements about the reaction must be true?
Le Chatelier’s Principle
In an esterification reaction, a carboxylic acid and an alcohol react to form an ester and water. This reaction establishes an equilibrium because the reverse process can also occur. If the water is allowed to boil and leave the system as water vapour, how will the equilibrium respond?