When heated, calcium carbonate goes through a chemical reaction, and produces calcium oxide (quick lime) powder and carbon
dioxide gas. a chemist performed this reaction in a lab and found that the mass of the calcium oxide (quick lime) was less than the
mass of the calcium carbonate. what is the reason behind this decrease in mass?
a. the carbon dioxide molecules produced were unstable and lighter in mass.
b. calcium oxide crystals produced break up at room temperature, leading to the difference in
c. carbon dioxide is produced, and as a gas, it was not captured to measure its mass.
d.
the calcium oxide crystals produced were unstable and lighter in mass.
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Part b: study of equilibrium on solubility: mg(oh)2(s) ⇌ mg2+(aq) + 2 oh–(aq) cloudy clear (pink) 7. a. b. 8. a. b. 9. 10. 11. 12. when adding concentrated hydrochloric acid, how did the appearance of the equilibrium mixture change? the change in appearance indicated a shift in the point of equilibrium. in which direction did the equilibrium shift? (l) left (r) right explain your answer to question 7a. you should indicate which ion was added to or removed from the equilibrium mixture. when adding edta, how did the appearance of the equilibrium mixture change? the change in appearance indicated a shift in the point of equilibrium. in which direction did the equilibrium shift? (l) left (r) right explain your answer to question 8a. you should indicate which ion was added to or removed from the equilibrium mixture. upon heating in which direction is the equilibrium shifting? upon cooling in which direction is the equilibrium shifting? is the forward reaction a. endothermic explain your answers to questions 9, 10, and 11. (l) left (r) right (l) left (r) right b. exothermic