Chem. Eq. ical Equilibrium Chem Record All Data and observations Here studying t
ID: 518385 • Letter: C
Question
Chem. Eq. ical Equilibrium Chem Record All Data and observations Here studying the Dissociation in Wat Eguilibrium ofHC2H Aci color of original equilibrium mixture: color change aftdr addition of NaC2Hao? Orange ge after heating mixture: low color change after cooling mixture: Orange m. Stud ng the IC MCouzos' libriul color of original equilibrium mixture: color change after addition of distilled water: pin b color change after addition of 12M HCl color change after addition of distilled water: pink color change after heating mixture: dark blue color change after cooling mixture: Pink ILL. Studying the Dissolution of NH n Water Equilibrium initial appearance of equilibrium mixture Clear change after addition of 12MHC: after heating mix that lehm peratu he appearanceExplanation / Answer
1. The following equilibrium is observed:
Co(H2O)62+(aq) + 4 Cl-(aq) <=> CoCl42-(aq) + 6 H2O(g)
The Co(H2O)62+ complex is pink, and the CoCl42- complex is blue.
When the NaClis added, Cl- is added to the equilibrium solution. the concentration of Cl ions is increased. Since, Cl is found on the product side, therefore there is an increase in products and the system shifts to the forward and produces more reactants (CoCl4-2 and H2O). This shifts the equation in forward direction, and the solution turns blue. When HCl is added, there is more Cl- in solution, so the equilibrium is shifted to the right, and the solution turns blue. The above effects are variations of LeChatelier's principle.
2. N2(g) + 3H2(g) 2 NH3(g)
A. forward reaction:
N2(g)+ 3H2(g) 2NH3(g)
b: backward reaction:
2NH3(g) N2(g) + 3H2(g)
Lechatlier's Principle: “If a chemical system at equilibrium experiences a change in concentration,temperature or total pressure, the equilibrium will shift in order to minimize that change.”
C. system has reached equilibrium : It means the rate of forward reaction is equal to rate of backward reaction.When this happens, the concentrations of nitrogen, hydrogen, and ammonia become constant, and the system is said to be “at equilibrium”
d. if we add N2 to equilibrium mixture the reaction : the equilibrium will move in forward direction towards the formation of more NH3. to produce more ammonia N2 reacts with Hydrogen. On increasing concentration of N2 necessarily the concentration of Hydrogen will decrease.
e. If we add NH3 to equilibrium mixture: Since there would be increase in the concentration of ammonia. Therefore the equilibrium will shift to left i.e backwards to dissociate into N2 and H2. thus, concentration of H2 will increase.
f. Change in concentration of N2 if we remove H2 from equilibrium mixture.: On removing hydrogen from equilibrium mixture the concentration of Hydrogen will be decreased. Therefore NH3 will dissociate more to increase the concentration of Hydrogen. Since, ammonia dissociates into N2 and H2 , the concentration of N2 will increase.
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