One question with 3 parts **Part B - Identify the impact on concentration**For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase:\[ \text{NH}_4\text{(aq)} + \text{OH}^-\text{(aq)} \rightleftharpoons \text{NH}_3\text{(aq)} + \text{H}_2\text{O(l)} \]**Drag the appropriate stresses to their respective bins.**- Adding OH⁻ (aq)- Removing NH₄⁺ (aq)- Adding NH₃ (aq)- Removing OH⁻ (aq)- Adding NH₄⁺ (aq)- **Shift in the direction of the reactants**- **Shift in the direction of the products**[Submit button]---**Equilibrium in the Human Body**The process of reaching equilibrium helps maintain the human body. Your overall health depends on your body’s ability to react appropriately to stress in order to rebalance biological functions. This process of maintaining biological balance is called homeostasis and it is similar to the way chemical equilibrium follows Le Châtelier’s principle.One example of an equilibrium reaction involved in homeostasis is oxygenation of the blood. This process is driven by an equilibrium between hemoglobin (Hb), oxygen (O₂), and oxyhemoglobin (HbO₂), and is represented by the equation:\[ \text{Hb(aq)} + \text{O}_2\text{(g)} \rightleftharpoons \text{HbO}_2\text{(aq)} \]---**Part C - Apply the method to an equilibrium reaction involved in homeostasis in biological organisms**As altitude increases, atmospheric pressure decreases. For instance, at 10,000 feet, your blood will obtain 25% less oxygen than you would at sea level, which means less oxygen in the blood from the lungs. This can lead to altitude sickness, or hypoxia as it is called.Imagine a mountain climber ascends to a tall peak, trying to climb Mount Kilimanjaro for the first time. The climber is very fit, so plans to summit in just 5 days. Use your knowledge of equilibrium to predict the climber’s reaction to this speedy climb, and the reactions needed to maintain equilibrium.**Match the equation to the appropriate blank in the sentences. **Foundations of Chemistry****Chapter 9: Problem-Solving Strategies: Understanding Equilibrium**---**Part A: Identify the Stress**Consider the equilibrium reaction:\[ \text{CO(g)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO}_2\text{(g)} + \text{H}_2\text{(g)} \]Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response to this stress.Drag the appropriate labels to their respective targets.**Diagram/Activity Box:**- **Left Panel (Changes and System Stress):** - **Decrease product**: Forward reaction rate temporarily increases. - **Decrease reactant**: Reverse reaction rate temporarily decreases. - **Increase reactant**: Reverse reaction rate temporarily increases. - **Increase product**: Forward reaction rate temporarily decreases.- **Right Panel (Changes, System Stress, and Equilibrium Shift):** - **Add CO\(_2\)**: - System Stress: Group 1 - Equilibrium Shift: Group 2 - **Remove H\(_2\)O\(_{(g)}\)**: - System Stress: Group 1 - Equilibrium Shift: Group 1 - **Add CO\(_{(g)}\)**: - System Stress: Group 2 - Equilibrium Shift: Group 2 - **Remove H\(_2\)O\(_{(g)}\)**: - System Stress: Group 2 - Equilibrium Shift: Group 1**Buttons:**- Submit- Request Answer---**Le Châtelier's Principle**In the first part of this tutorial, you analyzed why stressing a reaction by adding reactant or product would shift the equilibrium to create more reactant or more product. Adding more reactant increases the concentration of reactant, which increases the forward rate of reaction as equilibrium is re-established. Le Châtelier's principle is used to analyze this relationship.Le Châtelier’s principle applies to reversible reactions that are under some form of stress. Think of the equilibrium like a pile of laundry. If you add laundry on top of the pile, the additional pieces will roll down the pile and away from the source of the addition. This

Since you have asked multiple questions, we will solve the first one (Part A) for you. To get the…

▾ Part A-Identify the stress Consider the equilibrium reaction Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response CO(g) + H₂O(g) CO₂(g) + H₂(g) Drag the appropriate labels to their respective targets. Decrease product Decrease reactant Increase reactant Increase product Submit Request Answer Forward reaction rate Forward temporarily increases Reverse reaction rate temporarily decreases Reverse reaction rate temporarily increases Forward reaction rate temporarily decreases Change Add CO(g) Part B-Identify the impact on concentration Remove H₂O(g) Add CO₂(g) Remove H₂(g) System stress. Group 1 Group 1 Group 1 Group 1 Equilibrium shift Group 2 Group 2 Group 2 Reset Group 2 Help Le Châteller's principle n the first part of this tutorial you analyzed why stressing a reaction by adding reactant or product would shift the equilibrium to create more reactant or more product. Adding more reactant increases the concentration of reactant, which increases the forward rate of reaction as equilibrium is re- established. Le Châtelier's principle is used to analyze this relationship. <21 of 39 Châtelier's principle applies to reversible reactions that are under some form of stress. Think of the equilibrium like a pile of laundry. If you add more laundry on top of the pile, the additional pieces will roll down the pile and away from the source of the addition. This is similar to the equilibrium action that shifts away from a component addition. If you remove a piece of laundry from the bottom of the pile, however, the remaining laundry will fall in the direction of the removed piece. Therefore, the equilibrium shifts in the direction of the component that is removed For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase

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...