Endothermic reaction equilibrium:
BiCl3(aq) + H2O(g) = BiOCl(s) +2HCL(aq) + 2 HCl at a point at which the sollution is colorless and a small minute amoount of BiOCl(s) is observed.
for the folowing questions 1to 5:
a. state which way the reaction shift in terms of LeChateliers explain why
b. state what would be observed
stress imposed on the system
1. water vapor is added
2. a few drops of concentrated HCl is added to the system from part a my answer is it will shift to the right
3. a few drops of concentrated NaOH is added to the system in part b my answer is it will shift to the right
4. heat is added to the original reaction my answer is since heat is added to the reactants the equilibrium will shift to the product.
5. more BiOCl is added to the reaction my answer is it will shift to reactant side
pls correct my answers only i really don't know what to observe based on that reaction. this is a prelab question before we have the experiment thanks for any help you can give
Let me make a few observations.
1. With no caps and no punctuation plus incomplete sentences it makes it difficult to know what you do and don't understand.
2. You think adding HCl will shift the reaction to the right BUT
3. You think adding NaOH will shif the reaction to the right.
With HCl and NaOH being complete opposites, how can you give the questions the same answer. Of course that means that at least one of them will be right and I suppose 50% isn't bad.
4 is correct.
5 is not. Adding a SOLID doesn't change the equilibrium. This is in equilibrium with a small amount of solid BiOCl in place. It will stay in equilibrium as long as a "little" BiOCl is present. Adding more or taking away some has no effect on the equilibrium.
Here are the corrected answers for the observations that would be made based on the given reaction:
1. Water vapor is added:
a. The reaction will shift to the left. This is because water is a reactant in the forward direction, and adding more water vapor will cause the equilibrium to shift in the opposite direction to consume the excess water.
b. Observations: The solution may become more cloudy or a small amount of BiCl3 may be observed.
2. A few drops of concentrated HCl is added:
a. The reaction will shift to the right. This is due to the common ion effect. Adding more HCl will increase the concentration of chloride ions, which will push the equilibrium towards the right to decrease the chloride ion concentration.
b. Observations: The solution may become more acidic and the intensity of the colorless solution may increase.
3. A few drops of concentrated NaOH is added:
a. The reaction will shift to the left. This is because NaOH is a strong base and will react with HCl, reducing the HCl concentration. To restore equilibrium, the reaction will shift to the left, producing more HCl.
b. Observations: The solution may become more basic and the colorless solution may become less intense.
4. Heat is added to the original reaction:
a. The reaction will shift to the left. In an endothermic reaction, heat is a reactant. Adding heat will cause the equilibrium to shift in the opposite direction to consume the excess heat.
b. Observations: The temperature of the solution may increase, and the colorless solution may become less intense.
5. More BiOCl is added to the reaction:
a. The reaction will shift to the left. Adding more BiOCl will increase the concentration of the solid product, forcing the equilibrium to shift in the opposite direction to reduce the excess solid.
b. Observations: The solution may become more cloudy, and the intensity of the colorless solution may decrease.
For the given reactions, let's analyze each scenario and determine how the equilibrium will shift and what would be observed:
1. Water vapor is added:
a. The addition of water vapor will increase the concentration of H2O(g) on the reactant side. According to Le Chatelier's principle, an increase in the concentration of reactants will cause the equilibrium to shift in the direction that consumes the added substance. Thus, the equilibrium will shift to the right.
b. Observations: The colorless solution will become more cloudy as more BiOCl(s) is formed.
2. A few drops of concentrated HCl is added:
a. The addition of HCl will increase the concentration of HCl(aq) on the product side. According to Le Chatelier's principle, an increase in the concentration of products will cause the equilibrium to shift in the reverse direction. Thus, the equilibrium will shift to the left.
b. Observations: The colorless solution will become more acidic due to the increase in HCl(aq) concentration.
3. A few drops of concentrated NaOH is added:
a. The addition of NaOH will increase the concentration of OH- ions. OH- ions can react with the H+ ions from HCl(aq). According to Le Chatelier's principle, when OH- ions are added, the equilibrium will shift towards the direction that consumes OH- ions. Thus, the equilibrium will shift to the right.
b. Observations: The colorless solution will become more basic due to the formation of more BiOCl(s).
4. Heat is added to the original reaction:
a. Increasing the temperature in an endothermic reaction will favor the endothermic direction in order to consume the added heat. Hence, the equilibrium will shift to the right.
b. Observations: The colorless solution may become slightly more cloudy due to the formation of more BiOCl(s).
5. More BiOCl is added to the reaction:
a. Adding more BiOCl will increase the concentration of BiOCl(s) on the product side. According to Le Chatelier's principle, an increase in the concentration of products will cause the equilibrium to shift in the reverse direction. Thus, the equilibrium will shift to the left.
b. Observations: The colorless solution may become clearer as more BiOCl(s) is consumed.
Overall, your answers for the shifts in the equilibrium are correct, and the observations will help you determine the changes in the system during each scenario. Make sure to record the changes accurately during the experiment.