Determine Limiting Reagen Experiment

In this experiment, it is very important to ensure that the deionized water is just basic and not acidic in order to obtain accurate results. Calcium oxalate does not precipitate in an acidic solution because of the formation of H2C2O4-, an ion that does not precipitate with Ca2+ . Allowing the precipitate to settle is also very

In chemical reactions, the significance of knowing the limiting reactant is high. In order to increase the percent yield of product, increasing the limiting reactant, possibly, is the most effective. In this experiment we were able to calculate limiting reactants from the reaction of CaCl2. 2H2O + K2C2O4.H2O(aq).

In this experiment an elemental copper was cycled a series of five reactions where it ended with pure elemental copper as well, but at different stages of the cycle the copper was in different forms. In the first reaction, elemental copper was reacted with concentrated nitric acid where copper changed the form from solid to aqueous. Second reaction then converted the aqueous Cu2+ into the solid copper II hydroxide (Cu(OH)2) through reaction with sodium hydroxide. The third reaction takes advantage of the fact that Cu(OH)2 is thermally unstable. When heated, Cu(OH)2 decomposes (breaks down into smaller substances) into copper II oxide and water. When the solid CuO is reacted with sulfuric acid, the copper is returned to solution as an ion (Cu2+). The cycle of reactions is completed with the

For the experiment you will obtain an unknown sample, containing chloride ion, and perform the gravimetrical procedure using the sample of the analyte. An analyte is a chemical constituent that is determined from analytical techniques. The technique used in the experiment is the gravimetric determination analysis which is a method of quantitative chemical analysis in which the key constituent being sought after is converted to a substance that can be separated from the remaining sample. A common method for determining chloride ions involves isolating the silver chloride precipitate via filtration, determining its mass, and using stoichiometry to

If the relative amount of reactants is altered, then the limiting reactant may change accordingly. For example, a balanced chemical equation of a certain reaction specifies that an equal number of moles of two substances A and B is required. If there are more moles of B than of A, then A is the limiting reactant because it is completely consumed when the reaction stops and there is an excess of B left over.

The purpose of this lab was to use empirical evidence to determine the type of chemical change and be able to write these changes as balanced reactions. We found that 9 out of 16 reactions yielded precipitates and 1 had a color change (Cu(NO3)2 x KI). To set up this experiment, we combined different solutions in a well plate. 3 drops of Ca(NO3)2, Cu(NO3)2, Ni(NO3)2, and Zn(NO3)2 were put into wells A1 to A4, B1 to B4, C1 to C4, and D1 to D4 respectively. Next, 3 drops of KI, KOH, Na2C2O4, and Na2SO4 were placed in wells A1 through D1, A2-D2, A3-D3, and A4-D4 respectively.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

To ensure maximum efficiency and meet time constraints, the steps in the procedure were performed quickly and but carefully. Most binary mixings produced clear colorless solutions, milky white solutions, or white precipitates. The mixings of the known solutions were recorded in Matrix 1; half of the fields were blocked out to prevent repetitions and same mixtures. The table produced many notable observations; for instance, water produced clear colorless solutions in all mixings and mixings with lead (II) nitrate usually formed precipitates. To identify the unknown solutions, qualitative analysis was performed on the unknown solutions and compared with observations of known solutions in Matrix 1. For example, Unknown Solutions 3 and 9 were easily identified as potassium iodide because of its

And of course, human error such as the amount of the solution poured in, the exact amount of solutes in the solutions and the measurements taken. If this experiment were to be repeated, it should have stricter timing, identical testing materials and more careful

Crystals also formed on the bottom of the beaker as the concentration was not fully dissolved, settling to the bottom of the beaker. To improve the experiment, we could have used a better thermometer to record the appropriate data. We also should have heated the solution further to ensure the concentration of Copper Sulfate was

When one looks back at the procedure of the experiment, trials 1, 2, 3, 4, 5, and 6 all use 6 M HCl for their reactions, and if this were to be substituted for 6 M HNO3, then these reactions would have still taken place, except in trial 2 because copper is less reactive than hydrogen in all cases, but their final observations may yield different colored solids and solutions (Beran,

Of course, I could be wrong but we need not conclude superficially, that is without getting to know all the details about the formula.

The weakest feature of the paper is that although the formulas, presented by authors, are in general correct, but they do not support the conclusions the author extract from them, and mistake is hidden in the interpretation.

At the end of the experiment when the lid was removed, it was found out that the blue colour of the copper (II) sulphate solution has faded away. It was turned to pale grey and there were some precipitates present. It was the zinc powder that was in excess to ensure that the copper (II) sulphate solution could react fully with the zinc powder.

Before explaining the obtained results in details we start a summary on the intellectual merits and