SUMMARY
The equilibrium constant for the reaction of Calcium Carbonate (CaCO3) decomposing into Calcium Oxide (CaO) and Carbon Dioxide (CO2) at 500°C is determined using the equilibrium pressure of CO2, which is 1.2 x 10^-3 atm. The equilibrium expression for this reaction is based on the partial pressure of the gaseous product, CO2. The relationship between pressure and concentration is established through the ideal gas law, PV=nRT, allowing for the calculation of molarity from pressure. Therefore, the equilibrium constant (K) can be accurately calculated using the pressure of CO2 at the specified temperature.
PREREQUISITES
- Understanding of chemical equilibrium concepts
- Familiarity with the ideal gas law (PV=nRT)
- Knowledge of equilibrium constant expressions
- Basic principles of thermodynamics related to gas behavior
NEXT STEPS
- Calculate the equilibrium constant (K) for the reaction at 500°C using the provided pressure of CO2.
- Explore the relationship between pressure and concentration in gaseous reactions.
- Study the effects of temperature on equilibrium constants for various reactions.
- Investigate the implications of Le Chatelier's principle on the equilibrium of gas reactions.
USEFUL FOR
Chemistry students, chemical engineers, and researchers interested in thermodynamics and chemical equilibrium analysis.
