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The employed methodology involved the preparation of standard solutions and the solutions of varied concentration used in the spectrophotometer in order to determine the absorbance which has a linear relationship in the case the wavelengths are plotted against the concentrations. The latter are also directly connected with the initial change in equilibrium that has different values at different equilibrium. The result obtained could be the subject to human errors such as the preparation of standard solution, calculations and the instrument errors. The calculations finally resulted in 449627.606 the equilibrium constant for the experiment.

Introduction

Equilibrium is defined as a state of balance in which it ceases to be no observable changes in the chemical reaction processes. In the event that the chemical reaction achieves equilibrium, the quantity otherwise referred to as the concentration of the reactants becomes equal to the concentration of the products (Reger, Scott, and David 557). However, this is a phenomenon that is observed without applying any specific equipment. The truth of the situation, therefore, is that many reactions are taking place at the molecular levels as the products formed undergo reverse reactions so as to form reactants and vice versa. The experiment, therefore, is aimed at determining the equilibrium constant in relation to the rate constant and the factors which can affect the system that has achieved equilibrium (Reger, Scott David, 2010.p.557).

Equilibrium constant, on the other hand, assuming a chemical reaction

aA+bB cC+dD, with the implication that a, b, c and d represent the stoichiometric coefficients, A and B are the reactants, and C and D are the products constituting the reacting species at an identified or constant temperature, while the square brackets denote the concentrations in morality, then K=[C]c [D]d/ [A]a [B]b, such that K is the required equilibrium constant.

It can be inferred that the definition of equilibrium constant is based on the quotient in which the numerator is a factor product of the concentrations denoted by the square brackets of the products each raised to the power of its stoichiometric coefficient respective. The same technique is applied in the process of obtaining the denominator. The magnitude of equilibrium constant represents some relationships regarding the directions in which the reaction may tend to proceed forward. In the event that K becomes greater than one, the equilibrium opts to shift to the right, and, respectively, K of a magnitude less than one prompts the equilibrium to shift to the left (Kotz, Paul, and John 674). The significance of the equilibrium constant is thus to determine the direction in which a reaction proceeds provided that a reaction species is added or removed from the reaction. This may result in the reaction optimization and the production of high yields.

Methodology

Seven new dry test tubes were obtained, cleaned and labeled M, L, Std, 2, 3, 4, 5 respectively. To the first three test tubes accordingly, 3Ml of M nitrate, Potassium L, and MLx solutions were added. After that, a micropipette was used to add 1000 uL of M nitrate solution to the four numbered test tubes followed by the addition of the potassium L solution and the appropriate volumes of (uL), 600, 400, 200 and 0 respectively.

The four labeled reaction test tubes and de-ionized water were then employed for the analysis in which the spectrophotometer was used. The absorbance of the varied concentrations was then recorded against an operating frequency of 460nm. De-ionized water was used as a blank which had an expected zero reading. The absorbance of MLx was measured against the standard solution including the other four solutions in the four test tubes. Precautions that were taken include rinsing the cuvette twice with the solution to be measured. The cuvette was filled to the level line of the solution. Any liquid traces and fingerprints were cleaned, and finally the cuvette was placed in the sample compartment and absorbance was recorded to 3 decimal places.

Discussion

The equations of the chemical formula that are to be used for the calculations should be well balanced. The square brackets represent the concentrations in molarity, while the powers to which the concentrations are raised imply the stoichiometric coefficients in which case some time is taken in determination of the rate constants used to find the order of the reactions.

In relating concentration to the absorbance, there is the necessity to introduce the concept of the beer’s law. Concentration is directly proportional to the number of the molecules present in a given solution. Thus, the higher the number of the molecules in a reacting species, the higher the concentration which is directly proportional to an absorbance at given wavelength. Besides, it can be noticed that the increase in concentration is directly proportional to the absorbance. There was no addition of reaction species in the solution M, hence the reason for the constant concentration is the absence of any changes in the absorbance values. Absorbance is directly proportional to the concentration, therefore the concentrations obtained are used to draw parallels with the reference to the initial change equilibrium data table. One of the solutions, in this case solution M, with constant concentration is used as a standard reference upon which an average is obtained when a comparison to the standard equilibrium is made.

The uncertainties in the results obtained could arise from the defects of the instruments used, individuals inability to use the instruments properly, misleading concentration prepared from the stock solutions, as well as human error in executing mathematical operations. The sources of error can be avoided by following the instructions as outlined by the instructor and ensuring that instrumental and analytical machines used are modern and properly serviced. Human errors arising from the computations can be prevented through meticulously checking the results. The preparation of the correct concentration can be accomplished through application of the correct calculation formulae and ensuring that standard reagents are used.

Conclusion

The experiment provided an opportunity to determine the equilibrium constant of a given chemical reactions. To achieve relevant results, standard solutions must be prepared and references must be drawn from other measurements. A notable point to take into consideration is that, however, a chemical reaction may reach equilibrium, it does not mean that the experiment has come to a halt or a completion, but is of the implication that the reactions are proceeding at significantly slower rates.