The reaction below competes with the formation of the FeSCN^2+ complex: Fe^3+ (a

Question

The reaction below competes with the formation of the FeSCN^2+ complex: Fe^3+ (aq) + 4Cl^- (aq) FeCl^-_4 (aq) yellow colorless. Explain what would happen to the color of a dilute solution containing FeCl^-_4 if a. you added a solution containing silver ion, Ag^+. (Silver ion reacts with chloride ion in solution to form the precipitate AgCl.) b. you added a solution of sodium chloride, NaCl. c. you added concentrated HCl. d. you added concentrated H_3PO_4^-. Adding HCl or H_2SO_4/HPO^2^-_4 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) 2NH_3(g) + 22,000 cal. Consider the reaction is at equilibrium. Explain in which direction the equilibrium is shifted when a. more nitrogen is added? b. more hydrogen is added? c. ammonia is removed? d. the reaction is cooled?

Explanation / Answer

1)a) Adding Ag+ means removing Cl- from solution.Therefore, yellowishness will darken more.

b) Adding NaCl will remove excess Cl- by foforming FeCl4, therefore yellowishness will disappear

c) Similar to b) yellowness will disappear

d) Adding H3PO4 complex with Fe3+ and forms colorless solution.

2) Excess H+ ions will be in the solution if HCl/H2SO4 is added. Then by Lechatlier principle equilibrium will shift to left side or original side

3)a) when N2 is added , reaction favour products side

b) when H2 is added, reaction favour product side

c) when NH3 remove, once again it favour product formation

d) when cooled, reaction goes back to form reactants back

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