Question

(2) endothermic reaction to the solvo ions (3) Lo Châtelier's principle 3. A student is studying the equilibrium represented by the equaton 2 Cro/Taq, yellow) + 2 H3O"(aq) Cr2O72-"(aq, orange) + 3 H2O(i) The mixture abtained by the student is yellow EQUL 404/Studylt

Can you awnser all the questions above

Answer 1

3. A student is studying the equilibrium represented by the equation-

2CrO₄^2-(aq, yellow) +2H₃O+(aq) ---------à Cr₂O₇^2-(aq, orange) +3H₂O(l)

HCl is a strong acid so it dissociates into H⁺ ions and Cl- ions in solution. H⁺ does not exist in water; H⁺ ions will immediately react with water to produce H₃O⁺ ions. Therefore adding acid like HCl to the solution increases the concentration of H₃O⁺.

Le Chatelier's principle states that the reaction will shift to minimize this increase in H₃O⁺ shift away from additions, toward removals. So the reaction shifts to the right. Shifting to the right will increase orange dichromate in the solution, and solution will become orange.

5. Now, if excess NaOH is added to solution, it will consume H₃O⁺, reduce the reactants, shift left, and the solution will become yellow.

6. Write a net ionic equation to support answer 5-

  Cr₂O7^2- + 2OH^- + 2 H₃O⁺ ---> 2 CrO₄^2- + 3H₂O

7. OH^- reacts with H₃O⁺ to produce H₂O. La Chat says system will try and make more H₃O⁺ to counteract change and thus solution will go from orange to yellow.