The reaction below competes with the formation of the FesCN^2+ complex: Explain

Question

The reaction below competes with the formation of the FesCN^2+ complex: Explain what would happen to the color of a dilute solution containing FeCl_4^- if you added a solution containing silver ion, Ag^+ (Silver ion reacts with chloride ion in solution to form the precipitate AgCl.) you added a solution of sodium chloride, NaCl you added concentrated HCI. you added concentrated H_3PO_4 Adding HCl or H_2SO_4 to a mixture of H_2PO_4^-/HPO_4^2- would cause a common ion effect. What is the common ion, and what would be the overall observation? In which direction has the reaction shifted? The Haber process is an important reaction for the fixation of nitrogen; nitrogen is converted into ammonia, an important component in the production of fertilizers. N_2(g) + 3H)_2(g) rlarr 2NH_3(g) + 22 000 cal. Consider the reaction is at equilibrium. Explain in which direction the equilibrium is shifted when more nitrogen is added? more hydrogen is added? ammonia is removed? the reaction is cooled?

Explanation / Answer

1. For the given reaction,

Fe3+(aq) + 4Cl- --> FeCl4-(aq)

(yellow)                   (colorless)

a. When Ag+ is added, it reacts with Cl- to form AgCl precipitate. This would reduce concentration of Cl- in solution, thus according to LeChatellier's principle, more of colorless FeCl4- would go to form reactants Fe3+(yellow) and Cl-. Thus the color of solution would becomes more yellow.

b. When NaCl solution is added, Cl- concentration would increase, thus more of Fe3+ would reacts with excess Cl- added to form colorless FeCl4-. Color turns lighter.

c. concentrated HCl is added, Cl- concentration goes up, Fe3+ reacts with added Cl- to form more FeCl4-. Color of solution becomes lighter.

d. H3PO4 is a weak acid. No change on the color of the solution. It forms HCl, which is a strong acid and thus gives back Cl- to the solution.

2. Reaction,

H2PO4- <==> H+ + HPO4^2-

when HCl or H2SO4 is added, we have excess H+ in solution which is present on product end. Thus, the excess H+ would react with HPO4^2- in solution to form more H2PO4- species. The common ion being H+. the reaction equilibrium will shift towards the reactant side.

3. For the haber process

a. When more N2 is added, the equilibrium will shift to product side as excess N2 added would react woth H2 to form mor product NH3

b. When more H2 is added, the equilibrium will shift to product side as excess H2 added would react woth H2 to form mor product NH3

c. when NH3 is removed, the equilibrium will shift to product side as more N2 and H2 would react to reequilibriate the reaction condition to original state. More product NH3 would be formed.

d. Reaction is cooled, the equilibrium would shift towards product side. The reaction is exothermic in nature. A reduced temperature means reduced heat, so to reestablish equilibrium more heat has to be released and thus more products are formed.

These changes are according to the LeChatellier's principle.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.