Show the calculation of the theoretical yield of calcium carbonate. .0068 mol of CaCO3 *100. 06 g CaCO3/1mol of CaCO3 =. 6804 g of CaCO3 Show the calculation of the percent yield. (Actual yield/theoretical yield)*100 = (. 7/. 68)*100 =102% Conclusion: The objectives of this experiment were to use stoichiometry as a method to predict the amount of product produced from a precipitation reaction, to measure the reactants and products of the reaction with accuracy, and to discover the percent yield by calculating the actual yield and the theoretical yield
The mass of the weighing dish was measured as 0. g. The mass of the filter paper was measured as 1. 0 g. Initially it was calculated that 0. 68 g of CaCO3 was needed for a full reaction. The net mass of Na2CO3 (reactant) was 0. 72 g and the net mass of CaCO3 was 0. 7 g. The dried calcium carbonate measured at 0. 7 g (net mass).
The purpose of this experiment is to demonstrate a precipitation reaction combined with stoichiometry. The experiment also provided a method to improve substance measurement with utilizing measuring tools e. g. digital scales, beakers, and cylinders.
The Essay on Determining the limiting reactant and the percent yield i a precipitation reaction
One example of a double replacement (metathesis) reaction is the mixing of two solutions resulting in the formation of a precipitate. In solution chemistry, the term precipitate is used to describe a solid that forms when a positive ion (cation) and a negative ion (anion) are strongly attracted to one another. In this experiment, a precipitation reaction will be studied. Stoichiometry will then be ...
A Precipitation reaction begins by combining two aqueous solutions to form a precipitate, an insoluble product that is also a solid. Stoichiometry is a method that can be used with there is missing reactant data. Once the amount of the second reactant is found via the given amount of the first reactant, Stoichiometry also furthers exploration by providing a means of what to expect as the resulting product. Through this experiment it was discovered that stoichiometry can provide a means to decreasing calculation error with precipitate reactions.
To measure the distilled water, the 10 ml syringe was used to ensure precision. The scale was “zeroed out” with each use. However, this experiment was concluded with a 102% percent yield based on a 100% scale. Therefore there had to be experimental error. Due to the percent yield calculation it was concluded there had to be some Calcium Chloride, Dehydrate loss which could have affected the outcome of the Calcium Carbonate product. This could be due to multiple paper cup exchange which was a material malfunction.
To avoid this issue in future experiments home materials should be planned better and if possible tested to ensure functional needs are met. The issue could have come from weighing the final product and not “zeroing out” the scale before usage. To prevent this experimental error the scale should always be balanced before using. Rounding values during the calculation process could also add to the experimental error. In the future, significant figures should have a more dominant part in the calculation process.
