Conclusions for chemistry lab reports

Writing your lab reportworksheet - chemistry lab resources

Writing your lab reportworksheet - chemistry lab resources
Chemistry lab resources (for chm 1xx and 2xx labs) writing your lab reportworksheet.

Ice water is used as an absorber for the heat released in this reaction. Copper sulfate is a blue precipitate, but since it is soluble in water, it dissolves and the mixture is turned a bright blue color. The reaction that occurred in step 7 was a dehydration reaction. Unfortunately, that was not the case in this lab, and the final mass of copper exceeded the initial mass by 4. They must be independent units, accompanied by explanatory captions that allow them to be understood by someone who has not read the text.

As a result, the law of conservation of mass was still held true, and the same amount of copper that was used initially was also found in the final product of the reaction. The reaction between copper and nitric acid is an exothermic reaction. This states that in a chemical reaction, matter can neither be created or destroyed, or more simply, the mass of the products must equal the mass of the reactants. During the next step, error may have occurred if there was copper precipitate left on the side of the beaker instead of washed with water. The first step of the lab was to measure 2 g of copper and place it in a beaker.

The main chemical concept that this lab involves is the law of conservation of mass. We observe and record as objectively aspossible, avoiding personal bias by removing ourselves. Whether you are filling out lab worksheets or writing up entire lab reports, there are a few tips that will help you to create more detailed and professional documents and to assist in grading be aware of significant figures, noting the sensitivity of the device you are using for your measurements its part of the scientific point of view. You should limit the use of the past tense to (1) describe specific experimental methods and observations, and (2) citing results published in the past. The previous reaction that took place involved aqueous copper(ii) sulfate and solid zinc. Decanting also proposed a source of error because copper may have been accidentally lost, or not enough water may have been decanted from the beaker. In the final reaction, solid zinc was added to aqueous copper sulfate. The function of using the ice bath in this step is to control the temperature of the reaction, because the reaction may become too violent if nothing is used to cool it down. In this lab, we tested this by putting copper through five different reactions and many phase changes. Passive voice information derived from original work at delta college teachinglearning center purdue students explain strategies for dividing the workload for writing a lab report.

Copper lab - ap chemistry lab reports
The reaction between copper and nitric acid is an exothermic reaction. The function of using the ice bath in this step is to control the temperature of the.

Oct 21, 2016 lab reports are an essential part of all laboratory courses and a significant part of your grade. Heres a format for a lab report to use.

The function of using the ice bath in this step is to control the temperature of the reaction, because the reaction may become too violent if nothing is used to cool it down. Using the passive voice also clarifies proceduresand descriptions so they can be easily reproduced and compared. In the final reaction, solid zinc was added to aqueous copper sulfate. Law of conservation of mass, once this copper is returned to its original state, it will have the same mass. The reaction between zinc and sulfuric acid is as follows zn(s) h2so4(aq) --- znso4(aq) h2(g) when the cuo was washed, the excess hydroxide ions that could have remained from the previous reaction were removed.

We observe and record as objectively aspossible, avoiding personal bias by removing ourselves. During the next step, error may have occurred if there was copper precipitate left on the side of the beaker instead of washed with water. In this lab, we tested this by putting copper through five different reactions and many phase changes. There were many different sources of error throughout this lab, and i believe that this was the reason for such a significant difference between the initial and final masses and moles of copper that were calculated. Mass of evaporating dish and copper - mass of evaporating dish mass of copper final mass of copper x (moles of copper)(molar mass of copper) final moles of copper initial mass of copper x (moles of copper) (molar mass of copper) initial moles of copper percent yield (moles of copper recovered) (initial moles of copper) x 100 the initial mass of copper used in the experiment was 2.

Black precipitate is denser than water and sinks to the bottom of the beaker. The reaction between the excess zinc and sulfuric acid in step 9 is essential to ensure that there is so un-reacted solid zinc mixed in with the copper, and that any excess zinc is reacted to form zinc sulfate than is aqueous and can be poured out with water. If this was an incomplete reaction, there would be leftover solid zinc that would be weighed with the copper precipitate, and the zinc would increase the measured final mass of the copper and cause a significant difference between the initial and final masses of the copper. Ice water is used as an absorber for the heat released in this reaction. All in all, there was an abundance of sources of error in this lab. After finding the net ionic equation of the reaction, one determined that the products of the reaction were solid copper and aqueous zinc ions. This states that in a chemical reaction, matter can neither be created or destroyed, or more simply, the mass of the products must equal the mass of the reactants. If there was any solid zinc that did not react with the copper sulfate and was left over with the copper precipitate, zinc particles may have significantly changed the mass of the final product. So how did this happen? After going back and analyzing the reactions in the lab, we concluded that he majority of the sources of error in the lab would cause a loss of copper and a decrease in the final mass. In our lab, this was not the case, and we ended up with approximately three and one half times the amount of copper we started with, according to the law previously stated, this is impossible.

Parts of a lab report - chemistry lab resources for chm 1xx