Question

Which of the following would force the reaction to favor the products? CaCO3(s) + 2H3O(aq) + Ca(aq) + 3H2O(1) + CO2(g) A) Removing some of the H3O* from the reaction mixture B) Adding more Cal to the mixture C) Removing CO2 as it is formed D) Adding CO2 to the reaction mixture E) none of the above will have any effect on the amount of Cacos consumed 6. The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. What effect will be seen if the reaction temperature is raised? 3 NO(g) = N2O(g) + NO2(g) Han

Answer 1

Answer: Option (C) is the correct answer.

Explanation:

As the given reaction is as follows.

     $CaCO_{3}(s) + 2H_{3}O^{+}(aq) \rightleftharpoons Ca^{2+}(aq) + 3H_{2}O(l) + CO_{2}(g)$

According to Le Chatelier's principle, any disturbance caused in an equilibrium reaction will shift the equilibrium in a direction that will oppose the change.

Hence, in order to favor the formation of products when we remove $CO_{2}$ then there will occur decrease in it's concentration.

As $CO_{2}$ is forming on the product side and equilibrium will shift in the direction where there is less stress.

Hence, then equilibrium will shift in the forward direction, that is, on the products side.

Thus, we can conclude that removing $CO_{2}$ as it is formed would force the reaction to favor the products.