SUMMARY
The equilibrium constant (Kc) for the reaction involving 1.0 mol of N2O4(g) and 1.0 mol of NO2(g) in a 1.0 dm3 vessel, where 0.75 mol of N2O4(g) remains at equilibrium, is definitively calculated to be 3.0. The correct approach involves using the equilibrium concentrations of the reactants and products in the expression Kc = [NO2]2 / [N2O4]. The balanced chemical equation is N2O4(g) ⇌ 2NO2(g), confirming the stoichiometry used in the calculation.
PREREQUISITES
- Understanding of chemical equilibrium concepts
- Familiarity with the equilibrium constant (Kc) calculation
- Knowledge of stoichiometry in chemical reactions
- Ability to balance chemical equations
NEXT STEPS
- Review the principles of chemical equilibrium and Le Chatelier's principle
- Study the derivation and application of the equilibrium constant (Kc)
- Practice balancing chemical equations with varying stoichiometries
- Explore real-world applications of equilibrium constants in chemical reactions
USEFUL FOR
Chemistry students, educators, and anyone studying chemical equilibrium and reaction kinetics will benefit from this discussion.
