If the k value used in the experiment is lower than the actual constant, the calculated concentration of the solution will be lower than its actual value. This is because the absorbance values are directly related to the concentration of the solution through Beer's law.
Now, the Kc value is the equilibrium constant that represents the ratio of the concentrations of products to the concentrations of reactants raised to their respective stoichiometric coefficients in a balanced chemical equation. If the calculated concentration is lower than the actual concentration due to the lower k value used, the Kc value obtained in the experiment will be affected.
Depending on the Kc expression, specifically the stoichiometric coefficients and the number of terms involved, the deviation in Kc value may vary. If the stoichiometric coefficients are large or if there are multiple terms in the expression, the deviation in Kc value may be more significant.
Overall, using a lower k value in Beer's law would lead to an underestimation of the concentration values, which in turn would affect the calculated Kc value for the reaction. The extent of this deviation would depend on the specific Kc expression for the reaction being studied.
What would happen to Kc values in an experiment if the Beer's law constance (k) value used was low ( e.g you used 4000/M when the actual constant had a value of 5000/M)? Explain your answer
Absorbance = k*length cell*concentration
Cell length is constant.
You read an absorbance, so for any A read, plugging in k of 4000 instead of 5000 means the calculated concentration will be lower than it should be . What that does to Kc depends upon the Kc expression; i.e., the numerator and denominator (the number of terms and if any are raised to a power).
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