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The small x assumption applies when the equilibrium constant is small and initial reactant concentrations are sufficiently high, resulting in negligible conversion to products. This approximation simplifies calculations by treating the change in concentration as negligible. However, you must verify that x is less than 5% of the initial concentration to confirm the assumption's validity.

After solving for x using the simplified equilibrium expression, calculate the percentage change by dividing x by the initial concentration and multiplying by 100. If this percentage is less than 5%, the assumption is valid. If x exceeds 5% of the initial concentration, you must solve the problem again using the quadratic formula without making the approximation.

If x is greater than 5% of the initial concentration, the assumption is invalid and you cannot use the simplified equilibrium expression. Instead, you must rearrange the equilibrium expression into quadratic form and solve using the quadratic formula to obtain accurate equilibrium concentrations.

A small equilibrium constant indicates that the reaction produces very little product at equilibrium, meaning only a small fraction of reactants convert. When combined with high initial reactant concentrations, this ensures the change in concentration remains negligible, making the small x assumption mathematically sound and simplifying calculations significantly.

The assumption allows you to eliminate x from the denominator of the equilibrium expression. For example, if K = x²/(0.66 − x), you approximate (0.66 − x) as 0.66, yielding K = x²/0.66. This avoids the need to expand and solve a quadratic equation, making the calculation much faster and more straightforward.

The ICE table organizes Initial concentrations, Change in concentration (x), and Equilibrium concentrations for each species. It provides a systematic way to track how concentrations shift during the reaction and helps set up the equilibrium expression. The table clearly shows where the small x approximation is applied by treating the change as negligible.

Carbonyl dichloride has an extremely small equilibrium constant (2.2 × 10⁻¹⁰), meaning the reaction barely proceeds forward. With a high initial concentration of 0.66 M and such a small K value, only a tiny amount of reactant decomposes. The resulting x value of 1.2 × 10⁻⁵ M represents this minimal conversion, validating the small x assumption.