Math Problem Statement
Solution
The problem on the screen shows two reactions used to manufacture hydrogen, and it asks for the overall equilibrium constant in terms of the equilibrium constants and of the individual reactions.
Here are the reactions:
- with equilibrium constant
- with equilibrium constant
The overall reaction is:
To determine the overall equilibrium constant , you need to combine the two individual reactions.
Steps:
- The first reaction contributes to the formation of CO and hydrogen gas.
- The second reaction converts CO into CO2 and generates more hydrogen.
When combining equilibrium constants for sequential reactions:
- Multiply the equilibrium constants of the individual steps. So, the overall equilibrium constant is the product of and :
This gives the overall equilibrium constant for the net reaction.
Would you like further explanation or have any questions about the process?
Here are five related questions to expand understanding:
- How are equilibrium constants related to the Gibbs free energy of a reaction?
- What happens to the equilibrium constant if one of the reactions is reversed?
- How do temperature changes affect the equilibrium constant?
- How can Le Chatelier's principle be applied to these reactions?
- Can catalysts alter the equilibrium constant for a reaction?
Tip: When combining equilibrium constants from multiple reactions, ensure the direction of each reaction is consistent (i.e., if reversed, take the reciprocal of the constant).
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Math Problem Analysis
Mathematical Concepts
Chemical Equilibrium
Equilibrium Constants
Reaction Sequences
Formulas
K = K1 * K2
K = [Products]/[Reactants]
Theorems
Law of Mass Action
Equilibrium Constant Multiplication
Suitable Grade Level
High School (Grades 10-12), College Introductory Chemistry
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