8) To tube 6, add slowly 10 drops of water and place the test tube in a beaker o

Question

8) To tube 6, add slowly 10 drops of water and place the test tube in a beaker of ice. After 10 minutes, record the color you observe in tube 6 and any change in color. Questions 1) Consider the equilibrium reaction. NH3(g) + H2O(l) NH4+(aq) + (OH)-(aq) Describe whether the forward reaction or reverse reaction would be favored in the following scenarios. a) Mark adds five drops of o.1 M FeClh solution, which causes the formation of a brown Fe(OH)3 precipitate. b) Janet adds five drops of 1.0 M HCl, triggering a neutralization reaction that forms water through the consumption of hydroxide ions. c) Alan adds five drops of 0.2 MAgNOs, forming the diamminesilver (1) cation, [Ag(NHs)]. d) Laura adds five drops of 0.1 M KOH, adding more hydroxide to the solution. Conclusion Discuss some of what you learned about how changes in reaction conditions can have an impact on reaction rate and equilibrium.

Explanation / Answer

Hi dear Friend your answer as follows

a) During the formation of Fe(OH)3, FeCl3 consumes hydroxide ions (OH-), hence forward reaction would be favored to maintain equilibrium.
b) During the formation of water (H2O), H+ ions from HCl consumes hydroxide ions (OH-), hence forward reaction would be favored to maintain equilibrium.
c) During the formation of [Ag(NH3)2]2+, AgNO3 consumes ammonia (NH3), hence reverse reaction would be favored to maintain equilibrium.
d) During the formation of water (H2O), OH- ions consumes protons (H+), hence reverse reaction would be favored to maintain equilibrium.

Changes in reaction conditions is in accordance with Lechatlier's principle, which states that if an equilibrium is perturbed by varying the conditions like pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to counteract the change. This implies
1. If we increase concentration of reactants equilibrium shifts in forward direction to favor products.
2. If we increase concentration of products equilibrium shifts in reverse direction to favor reactants.
3. If we increase temperature of reaction which is exothermic by itself then equilibrium shifts to reverse direction to favor reactants.
4. If we increase temperature of reaction which is endothermic by itself then equilibrium shifts to forward direction to favor products.
5. If we increase pressure of reaction where the sum of product moles are lesser than sum of reactant moles then equilibrium shifts to forward direction to favor products.
6. If we decrease pressure of reaction where the sum of product moles are lesser than sum of reactant moles then equilibrium shifts to reverse direction to favor reactants.

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