Question

Which of the following would force the reaction to favor the produc to favor the products ? CaCO3(8) 2H3O'(aq) Cal(aq) + 3H200) + CO2(g) A) Removing some of the H2O 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 consumed c) none of the above will have any effect on the amount of CaCO3 consum The reaction of nitric oxide to form dinitrogen oxide and ritrogen dioxides exothermic. What effect will be seen if the reaction temperature is raised N2O(g) + NO2(g) AH 3 NO(9)

Answer 1

Explanation:

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

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

So, in this reaction when we any of the reactants then it means there is less stress on reactant side. Hence, the reaction will move in the backward direction.

Whereas when we remove $CO_{2}$ then there will be decrease in concentration of products as the concentration of carbon dioxide has decreased. Hence, the reaction will shift on the product side, that is, reaction will shift in the forward direction.

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

(b)   As the reaction equation is as follows.

            $3NO(g) \rightleftharpoons N_{2}O(g) + NO_{2}(g) + Heat$

Since, it is an exothermic reaction, that means when temperature is increasing then more amount of energy will release on the product side.

Hence, the reaction will shift on the reactant side, that is on the left hand side equilibrium will shift.