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Consider the following reaction at equilibrium. W(s) + 6 HCI(g) +WCls(g) + 3 H2(g) with AHo= 60 kJ What will happen to the H2 concentration in the following scenarios? HCI(g) is added? a) H2 will increase b) H2 will decrease c) Nothing will happen 20) W(s) is added? a) H2 will increase b) H2 will decrease c) Nothing will happen 21)

Consider the following reaction at equilibrium. W(s) + 6 HCI(g) +WCls(g) + 3 H2(g) with AHo= 60 kJ What will happen to the H2 concentration in the following scenarios? HCI(g) is added? a) H2 will increase b) H2 will decrease c) Nothing will happen 20) W(s) is added? a) H2 will increase b) H2 will decrease c) Nothing will happen 21)

Chemistry
Chemistry
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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
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### Chemical Equilibrium and Le Chatelier's Principle #### Consider the following reaction at equilibrium: \[ \text{W(s)} + 6 \text{HCl(g)} \leftrightarrow \text{WCl}_6\text{(g)} + 3 \text{H}_2\text{(g)} \; \text{with} \; \Delta H_0 = 60 \; \text{kJ} \] ### What will happen to the \( \text{H}_2 \) concentration in the following scenarios? 1. **HCl(g) is added** - a) \( \text{H}_2 \) will increase - b) \( \text{H}_2 \) will decrease - c) Nothing will happen 2. **W(s) is added** - a) \( \text{H}_2 \) will increase - b) \( \text{H}_2 \) will decrease - c) Nothing will happen ### Explanation of Potential Outcomes #### Scenario 1: Addition of HCl(g) When additional HCl(g) is added to the system, according to Le Chatelier's Principle, the equilibrium will shift to counteract this change. Adding more reactant (HCl gas) will shift the equilibrium to the right, thereby increasing the concentration of the products, including \( \text{H}_2 \) gas. - **Correct Answer: a) \( \text{H}_2 \) will increase** #### Scenario 2: Addition of W(s) Solid phases (W(s)) typically do not affect the equilibrium position in a reaction where they are present as a reactant or product because their concentration remains constant. - **Correct Answer: c) Nothing will happen** Understanding these reactions and their behaviors under various conditions is critical for mastering concepts in chemical equilibrium and the application of Le Chatelier's Principle.
Transcribed Image Text:### Chemical Equilibrium and Le Chatelier's Principle #### Consider the following reaction at equilibrium: \[ \text{W(s)} + 6 \text{HCl(g)} \leftrightarrow \text{WCl}_6\text{(g)} + 3 \text{H}_2\text{(g)} \; \text{with} \; \Delta H_0 = 60 \; \text{kJ} \] ### What will happen to the \( \text{H}_2 \) concentration in the following scenarios? 1. **HCl(g) is added** - a) \( \text{H}_2 \) will increase - b) \( \text{H}_2 \) will decrease - c) Nothing will happen 2. **W(s) is added** - a) \( \text{H}_2 \) will increase - b) \( \text{H}_2 \) will decrease - c) Nothing will happen ### Explanation of Potential Outcomes #### Scenario 1: Addition of HCl(g) When additional HCl(g) is added to the system, according to Le Chatelier's Principle, the equilibrium will shift to counteract this change. Adding more reactant (HCl gas) will shift the equilibrium to the right, thereby increasing the concentration of the products, including \( \text{H}_2 \) gas. - **Correct Answer: a) \( \text{H}_2 \) will increase** #### Scenario 2: Addition of W(s) Solid phases (W(s)) typically do not affect the equilibrium position in a reaction where they are present as a reactant or product because their concentration remains constant. - **Correct Answer: c) Nothing will happen** Understanding these reactions and their behaviors under various conditions is critical for mastering concepts in chemical equilibrium and the application of Le Chatelier's Principle.
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