llowing reaction produces chlorine molecules: + HCl (8) + CINO3 (8) Cl2 (8) + HNO3 (8) Describe 4 ways you could increase the concentratio How would cooling shift the equilibrium of this react are told that a chemical reaction is exothermic. How c
llowing reaction produces chlorine molecules: + HCl (8) + CINO3 (8) Cl2 (8) + HNO3 (8) Describe 4 ways you could increase the concentratio How would cooling shift the equilibrium of this react are told that a chemical reaction is exothermic. How c
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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Answer the question below please !!
![### Chemical Reactions and Equilibrium
**3) The following reaction produces chlorine molecules:**
\[ \text{Energy} + \text{HCl} \,_{(g)} + \text{ClNO}_3 \,_{(g)} \leftrightarrow \text{Cl}_2 \,_{(g)} + \text{HNO}_3 \,_{(g)} \]
**a) Describe 4 ways you could increase the concentration of chlorine molecules.**
1. **Increase the Concentration of Reactants:** Adding more hydrochloric acid (HCl) or chlorine nitrate (ClNO₃) to the system will shift the equilibrium to produce more chlorine (Cl₂).
2. **Increase the Temperature:** Since energy is a reactant, increasing the temperature adds more energy to the system, shifting the equilibrium towards the products and producing more chlorine molecules.
3. **Increase the Pressure:** For gas-phase reactions, increasing the system's pressure will shift the equilibrium towards the side with fewer moles of gas. If the reaction involves fewer moles of gas on the product side, increasing pressure will yield more Cl₂.
4. **Remove Products:** Continuously removing chlorine (Cl₂) or nitric acid (HNO₃) from the system will drive the reaction towards producing more products to replace them.
**b) How would cooling shift the equilibrium of this reaction?**
- Cooling the reaction would reduce the amount of energy available, which is a reactant in this case. According to Le Chatelier's principle, removing a reactant (in this case, energy) would shift the equilibrium towards the left to produce more reactants (HCl and ClNO₃), hence reducing the concentration of chlorine molecules (Cl₂).
**4) You are told that a chemical reaction is exothermic. How could you test whether the statement is true?**
- To test if a chemical reaction is exothermic, measure the temperature of the reaction mixture before and after the reaction. If the reaction is exothermic, it will release heat, and the temperature of the reaction mixture will increase.
- Additionally, you could use a calorimeter to precisely measure the heat released during the reaction. An exothermic reaction will show a negative change in enthalpy (ΔH < 0).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0fd17524-060d-4adb-8fd7-51abd298d44d%2Fef442229-66c3-4d3b-845b-3a98811ec8d9%2F3vabtw_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reactions and Equilibrium
**3) The following reaction produces chlorine molecules:**
\[ \text{Energy} + \text{HCl} \,_{(g)} + \text{ClNO}_3 \,_{(g)} \leftrightarrow \text{Cl}_2 \,_{(g)} + \text{HNO}_3 \,_{(g)} \]
**a) Describe 4 ways you could increase the concentration of chlorine molecules.**
1. **Increase the Concentration of Reactants:** Adding more hydrochloric acid (HCl) or chlorine nitrate (ClNO₃) to the system will shift the equilibrium to produce more chlorine (Cl₂).
2. **Increase the Temperature:** Since energy is a reactant, increasing the temperature adds more energy to the system, shifting the equilibrium towards the products and producing more chlorine molecules.
3. **Increase the Pressure:** For gas-phase reactions, increasing the system's pressure will shift the equilibrium towards the side with fewer moles of gas. If the reaction involves fewer moles of gas on the product side, increasing pressure will yield more Cl₂.
4. **Remove Products:** Continuously removing chlorine (Cl₂) or nitric acid (HNO₃) from the system will drive the reaction towards producing more products to replace them.
**b) How would cooling shift the equilibrium of this reaction?**
- Cooling the reaction would reduce the amount of energy available, which is a reactant in this case. According to Le Chatelier's principle, removing a reactant (in this case, energy) would shift the equilibrium towards the left to produce more reactants (HCl and ClNO₃), hence reducing the concentration of chlorine molecules (Cl₂).
**4) You are told that a chemical reaction is exothermic. How could you test whether the statement is true?**
- To test if a chemical reaction is exothermic, measure the temperature of the reaction mixture before and after the reaction. If the reaction is exothermic, it will release heat, and the temperature of the reaction mixture will increase.
- Additionally, you could use a calorimeter to precisely measure the heat released during the reaction. An exothermic reaction will show a negative change in enthalpy (ΔH < 0).
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