The reaction below competes with the formation of the FeSCN^2+ complex: Fe^3+ (a
ID: 1053013 • Letter: T
Question
The reaction below competes with the formation of the FeSCN^2+ complex: Fe^3+ (aq) + 4C^- (aq) FeCl_4^- (aq) 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 HCl. you added concentrated H_3 PO_4. Adding HCl or H_2 SO_4 to a mixture of H_2 PO_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) 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. (a) By adding silver ion, you are removing Cl- from solution. To counter this and re-establish equilibrium, some FeCl4- will decompose, forming Fe3+ and Cl-. The yellow colour will therefore deepen.
(b & c) Adding NaCl or concentrated HCl will cause the system to form FeCl4- to remove the excess Cl- ions, causing the yellow colour to fade or even disappear.
(d) Adding H3PO4 has a variety of effects. It complexes with the Fe3+ ions, turning them into a colourless complex. You will be removing the Fe3+ from the solution. The equilibrium will counter that by forming more Fe3+. However, you will always remove some Fe3+, meaning the colour will fade.
2. H2PO4- <====equilibrium====> HPO4-2 + H+
HCl -------------------> Cl + H+
HCl dissociates completely producing extra H+ in the solution of H2PO4-/HPO4-2. This solution before was already at equilibrium. Above that, adding extra H+ ions would change its equilibrium and degree of ionization (basically it would be reduced). Applying Le Chatelier's principle, the equilibrium will shift towards left to acheive new equilibrium with different concentrations.
H+ will be common ion since it is the one that is affecting equilibrium.
3.
A) According to Le Chatelier's principle, Increasing the amount of nitrogen at equilibrium will cause the equilibrium to move the right to get rid of it i.e by making more ammonia.
B.)use hydrogen and Nh3 is produced so shits right
C.) Removing ammonia will cause the equilibrium to move to the right to form more ammonia (decreasing the concentration of the reactants).
D.) The forward reaction is exothermic and the reverse is endothermic. So decreasing the temperature would result in the equilibrium moving in the exothermic direction to increase the temperature (i.e making more Ammonia), so right.
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