Math Problem Statement
Solution
The problem asks you to calculate the equilibrium constant for the given reaction at equilibrium:
The pressures of the gases at equilibrium are provided:
- : 72.5 atm
- : 57.3 atm
- : 34.1 atm
- : 61.6 atm
The equilibrium constant is calculated using the expression:
Where:
- is the equilibrium pressure of chlorine
- is the equilibrium pressure of water vapor
- is the equilibrium pressure of hydrogen chloride
- is the equilibrium pressure of oxygen
Substitute the given pressures:
Let's calculate:
- Multiply the numerator:
- Multiply the denominator:
- Now divide:
Rounded to two significant digits:
Let me know if you'd like any clarifications or further details!
Here are 5 related questions:
- How does the equilibrium constant change with temperature?
- What is the difference between and ?
- How would adding more affect the equilibrium of this reaction?
- Why are pressure values used instead of concentrations in this calculation?
- How does Le Chatelier's principle apply to this reaction?
Tip: Always double-check units when calculating equilibrium constants, as incorrect units can lead to wrong results.
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Math Problem Analysis
Mathematical Concepts
Equilibrium constants
Partial pressures
Formulas
Kp = (P_Cl2)^2 * (P_H2O)^2 / [(P_HCl)^4 * (P_O2)]
Theorems
Equilibrium law for gas-phase reactions
Suitable Grade Level
Undergraduate (College-level Chemistry)
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