Question

lab

Exploring Chemistry B. Reflective Exercises 1. In the carbonic acid equilibrium system, what happened to the size of the balloon upon the of more acid (HCI)? Was this expected? Why or why not? (Show your answer using the equilibrium equation) 2 Upon addition of NaOH to the equilibrium system, what happened to the size of the balloon? Was this expected?Why or why not? (Show your answer using the equilibrium equation.) 3. What direction of shift is expected with an endothermic reaction when heat is removed by decreasing the temperature of the system? heat + A + B C+D

Answer 1

Le Chatelier's principle says…

“changes to an equilibrium system will result in a predictable shift that will counteract the change”.

Means it acts in a reverse direction to neutralize the tension produced.

If it's a endothermic reaction, we know heat addition favors endothermic reaction i.e., heat act as a reactant here.

Le Châtelier's principle states that, when a change is made to a system that is already in equilibrium, the system reacts in such a way as to return to equilibrium. For a chemical reaction system, when the system "reacts so as to return to equilibrium", this means that the system will either react in the forward direction (so as to produce additional product) or in the reverse direction (so as to consume some of the product).

Ques 2  NaOH reacts with one of the components of the equilibrium, effectively removing that species from the equilibrium. NaOH is a strong base and reacts with acids: NaOH reacts with the hydrogen ion in the equilibrium system and removes it. If the H⁺ is removed from the equilibrium system, the system will have to react in the direction that replaces some of the H⁺ to restore equilibrium.

H⁺ (from the equilibrium) + OH^- (from the NaOH) = H₂O

The change in the system occurred when you added the NaOH, but the "stress" to the system must be described in terms of the equation for the equilibrium. since NaOH effectively removes hydrogen ion from the system by converting it to water, the "stress" from the equilibrium's point of view would be a decrease in the hydrogen ion concentration.

Fe³⁺ ion and SCN^- react with each other to form a red complex ion, [FeSCN]²⁺   .
Fe³⁺(colorless) + SCN^- (colorless) = [FeSCN]²⁺ (blood red)

In this system, we can tell in which direction the equilibrium shifts when a change is made by monitoring the intensity of color of the system. If the system gets darker red in color, then the equilibrium must be shifting to the right (toward producing more of the colored product). If the color of the system gets fainter (or disappears altogether), the equilibrium must be shifting toward the left (toward the colorless components).

• Equilibrium is a dynamic process at the molecular level. There is no net change, but two opposing processes are taking place.
• The equilibrium constant fluctuates slightly due to unequal reaction rates in opposite directions.
• A system moves spontaneously toward a state of equilibrium.
• The driving forces for equilibrium are:
  (a) molecules assume the state of lowest energy,
  (b) molecules tend to reach a maximum disorder or entropy.
• Equilibrium state is a dynamic balance between the forward and backward reaction.
• Dynamic Equilibrium

At dynamic equilibrium, reactants are converted to products and products are converted to reactants at an equal and constant rate. Reactions do not

It's dynamic because the reaction is still happening, but the reverse reaction is occurring at the same rate as the forward reaction, so the net change in the system is equal to zero. Think of it like your kitchen sink without a plug. If you put water into it (forward) at the same rate water drains out (reverse) then the level of the water will always be the same, even though you're filling and draining.

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