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?
World of Chemistry, 3rd edition
3rd Edition
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 38A
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Please help! I have seen three different ways to solve this and am so confused!
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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60db8604-0682-4af2-aa94-1f9fd1bb47db%2F1a3f2408-1ba6-432a-b3bf-68e102d14498%2F73va3eo_processed.png&w=3840&q=75)
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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