Question

Consider the following reaction at equilibrium, CaCO₃(s) ↔ CaO(s) + CO₂(g). Which of the following statements are true regarding this equilibrium?

Select all that are True.
a) If CaO(s) is added from the equilibrium mixture the reaction will remain unchanged.
b) If CaO(s) is removed from the equilibrium mixture the reaction will shift to the left.
c) If CO2(g) is added to the equilibrium mixture the reaction will shift to the right.
d) If CO₂(g) is added to the equilibrium mixture the reaction will shift to the left.
e) If CaCO₃(s) is removed to the equilibrium mixture the reaction will shift to the left.

Answer 1

solution. - GCO3 (6) - Go (so + CO2 g Effect on equilibrung s y Gog is added from the equili breins mixture the mactions will remain unchanged True) Reason. According to be chattier's principle, change in concentrates al solid reactant or product has negligibl effect on equilibrems Conditiers. b) af GO so is removed from the equilibrium mixture, the reacteers will shift to the left false)

c) y CO2 eg is added to the equilibrum mixture the reaction will shift to the right I false) Reason. According to de Chatelier's Principle, addits af products at equilibrum will shift equilibrium to the left y Corg is added to the equilibrum mistere the reaction will shift to the left True) Resson! - This is according to de Chattiers frinupple e) y GCO3 is removed to the equili bruns mixture the reactions will sheft to the right Reason! - recording to de Chatelier's Principle, additers ar removal al solid reactan 5 or Products has insignifiant effeil on equilibrin

Answer 2

true

false

false

true

false