SUMMARY
The equilibrium concentration of CO in the reaction CO(g) + NH3(g) → HCONH2(g) at 400K is determined using the equilibrium constant K = 0.207. Given initial concentrations of 2.20 M for CO and 2.60 M for NH3, the equilibrium concentration of CO is calculated to be 0.44 M. The calculation involves solving the equation 0.207 = (X) / ((2.20 - X)(2.60 - X)), leading to the valid root of 1.76 for X, which results in a positive concentration for CO.
PREREQUISITES
- Understanding of chemical equilibrium concepts
- Familiarity with equilibrium constant expressions
- Ability to solve quadratic equations
- Knowledge of concentration units in molarity (M)
NEXT STEPS
- Study the derivation of equilibrium constant expressions for different reactions
- Learn how to graph quadratic equations to find roots
- Explore the impact of temperature on equilibrium constants
- Investigate Le Chatelier's principle and its applications in chemical reactions
USEFUL FOR
Chemistry students, educators, and professionals involved in chemical reaction analysis and equilibrium calculations will benefit from this discussion.