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Activity 4 Kc and K, Directions: Write the equilibrium constant expression (Ke and K, ) for the following reactions: 1. 2SO2 (2 + 02 g = 2SO3 ()

Activity 4 Kc and K, Directions: Write the equilibrium constant expression (Ke and K, ) for the following reactions: 1. 2SO2 (2 + 02 g = 2SO3 ()

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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Acttivity 4 

Numbers 1 and 2 

2. 2ZnS + 302 ( = 2ZnO + 2SO2 Processing Question 1. What factors can affect systems in equilibrium? INTEGRATION Reflection Guide 1. How do you value academic proficiency in answering this module? INTERVENTION Post - assessment It's now time to assess your learning. If you do well, you may move on to the next lesson. If your score is not at the expected level, you may talk to your subject teacher to go back with the lesson and for you to be given remedies to cope up and understand the lesson. Directions: Read the following questions below. Circle the letter that corresponds to the correct answer. 1. In case of nonspontaneous reaction, the reaction favoured is C. both forward and reverse D. reaction stops A. Forward B. Reverse 2. In which of the following physical states does a given substance have the highest entropy? A. Solid B. Gas C. liquid D. entropy is the same 3. What are the two factors that determine whether a reaction is spontaneous or nonspontaneous? A. Entropy and disorder B. Entropy and enthalpy change C. electron configuration and charge D. energy and the heat of reaction 4. The amount of disorder in a system is measured by its A. Activation energy B. Entropy C. equilibrium position D. Keq 5. Which of the following refers to all spontaneous processes? A. Are exothermic B. Are endothermic C. involve an increase in entropy D. release free energy Page | 8
Transcribed Image Text:2. 2ZnS + 302 ( = 2ZnO + 2SO2 Processing Question 1. What factors can affect systems in equilibrium? INTEGRATION Reflection Guide 1. How do you value academic proficiency in answering this module? INTERVENTION Post - assessment It's now time to assess your learning. If you do well, you may move on to the next lesson. If your score is not at the expected level, you may talk to your subject teacher to go back with the lesson and for you to be given remedies to cope up and understand the lesson. Directions: Read the following questions below. Circle the letter that corresponds to the correct answer. 1. In case of nonspontaneous reaction, the reaction favoured is C. both forward and reverse D. reaction stops A. Forward B. Reverse 2. In which of the following physical states does a given substance have the highest entropy? A. Solid B. Gas C. liquid D. entropy is the same 3. What are the two factors that determine whether a reaction is spontaneous or nonspontaneous? A. Entropy and disorder B. Entropy and enthalpy change C. electron configuration and charge D. energy and the heat of reaction 4. The amount of disorder in a system is measured by its A. Activation energy B. Entropy C. equilibrium position D. Keq 5. Which of the following refers to all spontaneous processes? A. Are exothermic B. Are endothermic C. involve an increase in entropy D. release free energy Page | 8
2. PNH3 Kp PN2PH2 %3D 3. [N21 [H2]3 Heterogeneous Equilibria A heterogeneous equilibrium consists of reactants and products that exist in different phases. An example is the CACO3 (9) = Ca0 9 + CO2 (3) In a heterogeneous equilibrium, pure solid and liquid substances do not appear in the equilibrium constant expression. The molar concentrations of these substances are always constant (having a value equal to 1). The values are then not incorporated in the equilibrium constant expressions. For the calcium carbonate equilibrium reaction, the K K = [CO2] K, = Pco2 %3D %3D pue Le Chatelier's Principle V A system will adjust to regain its equilibrium if stress is applied to it. Le Chatelier's principle states that when stress is introduced into a system in equilibrium, the system will adjust to relieve the stress and regain equilibrium. The stress is relieved as the reaction shifts either to the left (reverse) or to the right (f of the reversible reaction. One factor that can affect systems in equilibrium is the change in the amount of either the reactants or the products. Adding more reactants to a reaction that is already in equilibrium will cause it to shift to the right. Adding more producis will favour the reverse reaction. Activity 4 Ke and K, Directions: Write the equilibrium constant expression (K. and K, ) for the following reactions: 1. 2SO2 (2) + 02 ( = e 2SO3 (g) Page | 7
Transcribed Image Text:2. PNH3 Kp PN2PH2 %3D 3. [N21 [H2]3 Heterogeneous Equilibria A heterogeneous equilibrium consists of reactants and products that exist in different phases. An example is the CACO3 (9) = Ca0 9 + CO2 (3) In a heterogeneous equilibrium, pure solid and liquid substances do not appear in the equilibrium constant expression. The molar concentrations of these substances are always constant (having a value equal to 1). The values are then not incorporated in the equilibrium constant expressions. For the calcium carbonate equilibrium reaction, the K K = [CO2] K, = Pco2 %3D %3D pue Le Chatelier's Principle V A system will adjust to regain its equilibrium if stress is applied to it. Le Chatelier's principle states that when stress is introduced into a system in equilibrium, the system will adjust to relieve the stress and regain equilibrium. The stress is relieved as the reaction shifts either to the left (reverse) or to the right (f of the reversible reaction. One factor that can affect systems in equilibrium is the change in the amount of either the reactants or the products. Adding more reactants to a reaction that is already in equilibrium will cause it to shift to the right. Adding more producis will favour the reverse reaction. Activity 4 Ke and K, Directions: Write the equilibrium constant expression (K. and K, ) for the following reactions: 1. 2SO2 (2) + 02 ( = e 2SO3 (g) Page | 7
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