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Consider the following reversible reaction to answer questions 1-4. It is EXOTHERMIC. 2 CO2 (g) 4 2 CO (g) + O2 (g) 1. Write the Kexpression for this balanced equation. 2. If, at equilibrium, the concentrations of the reactants and products are as follows: [CO] = 0.00025 M, [O2] = 0.00050, [CO2] = 0.25 M, calculate the value for Ko 3. Where does the equilibrium lie, towards the products or reactants? How can you know?

Consider the following reversible reaction to answer questions 1-4. It is EXOTHERMIC. 2 CO2 (g) 4 2 CO (g) + O2 (g) 1. Write the Kexpression for this balanced equation. 2. If, at equilibrium, the concentrations of the reactants and products are as follows: [CO] = 0.00025 M, [O2] = 0.00050, [CO2] = 0.25 M, calculate the value for Ko 3. Where does the equilibrium lie, towards the products or reactants? How can you know?

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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b. Add a catalyst C. Increase volume d. Remove O2 e. Remove CO2 f. Lower the temperature g. Add pressure h. Add heat
Transcribed Image Text:b. Add a catalyst C. Increase volume d. Remove O2 e. Remove CO2 f. Lower the temperature g. Add pressure h. Add heat
Consider the following reversible reaction to answer questions 1-4. It is EXOTHERMIC. 2 CO2 (g) = 2 CO (g) + O2 (g) 1. Write the Kexpression for this balanced equation. 2. If, at equilibrium, the concentrations of the reactants and products are as follows: [CO] = 0.00025 M, [O2] = 0.00050, [CO2] = 0.25 M, calculate the value for Ko 3. Where does the equilibrium lie, towards the products or reactants? How can you know? 4. How would the equilibrium system respond to the following stresses? Towards products, reactants or no change? Stress Shift? a. Add more CO
Transcribed Image Text:Consider the following reversible reaction to answer questions 1-4. It is EXOTHERMIC. 2 CO2 (g) = 2 CO (g) + O2 (g) 1. Write the Kexpression for this balanced equation. 2. If, at equilibrium, the concentrations of the reactants and products are as follows: [CO] = 0.00025 M, [O2] = 0.00050, [CO2] = 0.25 M, calculate the value for Ko 3. Where does the equilibrium lie, towards the products or reactants? How can you know? 4. How would the equilibrium system respond to the following stresses? Towards products, reactants or no change? Stress Shift? a. Add more CO
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