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Consider this reaction: Na(e) + 3H2(e) <----> 2NH3(2) H=-123KJ Describe how the concentration of H2 will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease or not chang a) The volume of the reaction chamber is decreased b) Helium gas is added to the reaction chamber. c) The temperature is increased. d) N, has is added to the reaction chamber.

Consider this reaction: Na(e) + 3H2(e) <----> 2NH3(2) H=-123KJ Describe how the concentration of H2 will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease or not chang a) The volume of the reaction chamber is decreased b) Helium gas is added to the reaction chamber. c) The temperature is increased. d) N, has is added to the reaction chamber.

Chemistry
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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Please answer c and d

**Chemical Equilibrium and Le Chatelier's Principle** Consider this reaction: \[ N_2(g) + 3H_2(g) \leftrightarrow 2NH_3(g) \quad \Delta H = -123 \text{kJ} \] ### Reaction Description The reaction depicted above is the synthesis of ammonia from nitrogen and hydrogen gases, also known as the Haber-Bosch process. This process is exothermic, releasing 123 kJ of energy. ### Equilibrium Effects on H₂ Concentration Describe how the concentration of \( H_2 \) will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease, or not change? a) **The volume of the reaction chamber is decreased** b) **Helium gas is added to the reaction chamber** c) **The temperature is increased** d) **\( N_2 \) gas is added to the reaction chamber** #### Explanation: 1. **Decrease in Volume**: - **Effect**: Decreasing the volume increases pressure. - **Shift**: According to Le Chatelier's Principle, the system will shift towards the side with fewer gas molecules to reduce pressure. - **Result**: The reaction shifts to the right (towards producing \( NH_3 \)), decreasing the concentration of \( H_2 \). 2. **Addition of Helium Gas**: - **Effect**: Adding an inert gas like helium at constant volume increases total pressure but does not change the partial pressures of the reacting gases. - **Shift**: There is no shift in the equilibrium position. - **Result**: The concentration of \( H_2 \) will not change. 3. **Increase in Temperature**: - **Effect**: Increasing temperature adds heat to the system. - **Shift**: Since the reaction is exothermic (\( \Delta H < 0 \)), increasing temperature shifts the equilibrium to the left (towards reactants). - **Result**: The concentration of \( H_2 \) will increase. 4. **Addition of \( N_2 \) Gas**: - **Effect**: Adding \( N_2 \) increases the concentration of one of the reactants. - **Shift**: The equilibrium will shift to the right to consume the additional \( N_2 \
Transcribed Image Text:**Chemical Equilibrium and Le Chatelier's Principle** Consider this reaction: \[ N_2(g) + 3H_2(g) \leftrightarrow 2NH_3(g) \quad \Delta H = -123 \text{kJ} \] ### Reaction Description The reaction depicted above is the synthesis of ammonia from nitrogen and hydrogen gases, also known as the Haber-Bosch process. This process is exothermic, releasing 123 kJ of energy. ### Equilibrium Effects on H₂ Concentration Describe how the concentration of \( H_2 \) will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease, or not change? a) **The volume of the reaction chamber is decreased** b) **Helium gas is added to the reaction chamber** c) **The temperature is increased** d) **\( N_2 \) gas is added to the reaction chamber** #### Explanation: 1. **Decrease in Volume**: - **Effect**: Decreasing the volume increases pressure. - **Shift**: According to Le Chatelier's Principle, the system will shift towards the side with fewer gas molecules to reduce pressure. - **Result**: The reaction shifts to the right (towards producing \( NH_3 \)), decreasing the concentration of \( H_2 \). 2. **Addition of Helium Gas**: - **Effect**: Adding an inert gas like helium at constant volume increases total pressure but does not change the partial pressures of the reacting gases. - **Shift**: There is no shift in the equilibrium position. - **Result**: The concentration of \( H_2 \) will not change. 3. **Increase in Temperature**: - **Effect**: Increasing temperature adds heat to the system. - **Shift**: Since the reaction is exothermic (\( \Delta H < 0 \)), increasing temperature shifts the equilibrium to the left (towards reactants). - **Result**: The concentration of \( H_2 \) will increase. 4. **Addition of \( N_2 \) Gas**: - **Effect**: Adding \( N_2 \) increases the concentration of one of the reactants. - **Shift**: The equilibrium will shift to the right to consume the additional \( N_2 \
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