Question

» What color did you observe after adding the 3M H2SO, solution? 4) What color did you observe after adding the IM NaOH solution? Assume that the dynamic equilibrium represented in the equation in I is present in the original solution you placed in the test tube. Based on LeChatelier's Principle, as stated above on page one, you will interpret the observations made in 2, above: (Note that H SO, produces H+ in solution.) a) When sulfuric acid was added, which reaction (forward or reverse) was favored? What evidence supports this? Why would this reaction be favored? b) Assume that the system rapidly returns to equilibrium. At this new position of equilibrium, is there more or less Cr 07 present after the addition of the acid? Based on this, what happened to the amount of C10.2? Dosto Before answering the next question, consider this: Even before acid was added, the amounts of the two chromium ions were not equal.(Remember equilibrium means equal rates, not equal amounts.) c) If the amount of one of these ions increased and the amount of the other decreased, how is it that the rates of the forward and reverse reactions come to be equal again? (Hint: Assume the rate of the forward reaction is kr [H][ CrO2) and that of the reverse reaction is k. [Cr:07] wa boss do not Omit this questi 6) Based on LeChatelier's Principle, as stated above, you will interpret the observations made in 3. above: Note: NaOH produces OH-in solution. a) When sodium hydroxide was added, which reaction in 1 (forward or reverse) was favored? What evidence supports this? Why would this reaction be favored? (Hint: What does OH- do with H+?) b) Assume that the system rapidly returns to equilibrium. After the addition of the NaOH, at this new position of equilibrium, is there more or less Cr207 present? Based on this, what happened to the amount of Cro?? COD

Answer 1

Ah8 6 2 crog ² + 2H+ Groq² +th a) when Naon was added then on increaze which react with it and form tho. So the concentration of it will be decreazed after adding NaOH solution. So the reaction goes in back weard direction. Accarding to he chattlier's principle Equilibrium tends to nullify the count eraet. b) when Noon is also added then the Equilibirium will tends in the backward of the reaction goes in backward direction then the concentration of coeg op 2- is also decreaze. If yo, 2- concentration decreazed then the concentration of Groor is also In creazed. This is a perfeet application of Le Chattlier's principle. ion Scanned with CamScanner