Please specify the answers need them to study **Topic:** Le Chatelier's Principle and Chemical Equilibrium**Overview:** An analysis of the changes in equilibrium for the reaction $2\text{H}_2\text{S(g)} \rightleftharpoons 2\text{H}_2(g)} + \text{S}_2(g)}$, which is endothermic.**i. Decreasing the Temperature:**- **Effect:** Shifts to the right.- **Explanation:** Lowering the temperature of an endothermic reaction favors the formation of products, shifting equilibrium to the right.**ii. Adding a Catalyst:**- **Effect:** No effect.- **Explanation:** Catalysts speed up the rate at which equilibrium is achieved but do not change the position of the equilibrium.**iii. Removing $\text{H}_2(g)$:**- **Effect:** Shifts right.- **Explanation:** Removing a product from the reaction shifts the equilibrium towards the products to replace what was removed.**iv. Adding $\text{H}_2\text{S(g)}$:**- **Effect:** Shifts right.- **Explanation:** Adding more reactants causes the equilibrium to shift towards the products to balance the change.**v. Decreasing the Volume of the Reaction Container:**- **Effect:** Shift to the left, favoring the side with more moles.- **Explanation:** Decreasing volume increases pressure; the reaction shifts towards the side with fewer moles of gas to reduce pressure. Understanding these principles helps predict how changes affect chemical systems, crucial for controlling industrial reactions and processes.

The given endothermic reaction is: 2H2S(g) ⇌ 2H2(g) + S2(g) According to Le-Chatelier's principle, when a chemical reaction in equilibrium undergoes a change, the reaction moves in such a way that it is able to nullify the change. #(i): Since this is an endothermic reaction, heat is required to complete the reaction i.e heat is on the reactant side. When we decrease the temperature, the heat on the reactant side decreases. Hence the reaction moves to the reactant side so that the heat increases. Hence the reaction shifts to the reactant side (left side). (Answer) #(ii): A catalyst only helps to reach the equilibrium faster, but it doesn't affect the equilibrium position. Hence adding a catalyst has no effect at equilibrium (Answer) #(iii): When we remove H2(g), the product concentration decreases. Hence the reaction moves towards the product side so that the product concentration would increase. Hence the reaction shifts to the right side (product side) # (iv): When we add H2S(g), the reactant concentration increases. Hence the reaction moves towards the product side so that the reactant concentration would decrease. Hence the reaction shifts to the right side (product side)#(v): Decreasing the volume increases the pressure. Due to an increase in pressure, the number of gaseous molecules per unit volume increases. Hence the reaction moves in a direction where the number of gaseous moles decreases. Since the reactant side has smaller number of gaseous moles, the reaction moves to the left side (reactant side). Hence the reaction moves to the left side (reactant side).

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d. The reaction (2H2S(g) 2H2(g) + S2(g)) is endothermic. Describe the effect of the following changes on the equilibrium: i. Decreasing the temperature. Shifts to the right ii. Adding a catalyst. no effect iii. Removing H2(g). Shifts right iv. Adding H2S(g) Shifts rignt v. Decreasing the volume of the reaction container (Hint: what happens to the pressure?) shift to left faver Of gab wtn more moles

d. The reaction (2H2S(g) 2H2(g) + S2(g)) is endothermic. Describe the effect of the following changes on the equilibrium: i. Decreasing the temperature. Shifts to the right ii. Adding a catalyst. no effect iii. Removing H2(g). Shifts right iv. Adding H2S(g) Shifts rignt v. Decreasing the volume of the reaction container (Hint: what happens to the pressure?) shift to left faver Of gab wtn more moles

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Please specify the answers need them to study

**Topic:** Le Chatelier's Principle and Chemical Equilibrium

**Overview:** An analysis of the changes in equilibrium for the reaction $2\text{H}_2\text{S(g)} \rightleftharpoons 2\text{H}_2(g)} + \text{S}_2(g)}$, which is endothermic.

**i. Decreasing the Temperature:**
- **Effect:** Shifts to the right.
- **Explanation:** Lowering the temperature of an endothermic reaction favors the formation of products, shifting equilibrium to the right.

**ii. Adding a Catalyst:**
- **Effect:** No effect.
- **Explanation:** Catalysts speed up the rate at which equilibrium is achieved but do not change the position of the equilibrium.

**iii. Removing $\text{H}_2(g)$:**
- **Effect:** Shifts right.
- **Explanation:** Removing a product from the reaction shifts the equilibrium towards the products to replace what was removed.

**iv. Adding $\text{H}_2\text{S(g)}$:**
- **Effect:** Shifts right.
- **Explanation:** Adding more reactants causes the equilibrium to shift towards the products to balance the change.

**v. Decreasing the Volume of the Reaction Container:**
- **Effect:** Shift to the left, favoring the side with more moles.
- **Explanation:** Decreasing volume increases pressure; the reaction shifts towards the side with fewer moles of gas to reduce pressure.

Understanding these principles helps predict how changes affect chemical systems, crucial for controlling industrial reactions and processes.

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