Stoichiometry Lab Report

In order to find the amount of a product made during a double displacement reaction, the product has to be separated from the solution. From this number of moles of precipitate can be calculated. From there the number of moles of reactants can be calculated using the mole ratios of the particular reaction that occurred. As seen in Table 5 it is shown that by finding out the number of moles of the unknown, the molar mass of the unknown can be calculated. From the found mass of the unknown compound, the mound of the original ion can be found.

In the end, my results were very close to the actual values, which produced my low percent error of -3.0%. In conclusion, this lab experiment went well. I completed the objectives successfully, concluding with fairly accurate data, and thus a low percent error. However there is a small space for improvement within the construction of this lab, which possibly could have prevented the negative error I obtained.

In order to observe oxygen consumption exclusively, NaOH was utilized to absorb carbon dioxide. An absorbent cotton ball saturated with one molar NaOH was placed on the bottom of each vial, followed by a non-absorbent cotton ball in order to ensure the chemical

The equation used to determine the molar mass is derived from the Ideal Gas Law equation. The objective of this experiment aims to determine the molecular mass of a

This finding could have been due to experimental errors which affected the results. Discussion

The general formula is below, where the determined moles of base from the equation above are multiplied by the stoichiometric ratio found by looking at the balanced

Multiple experiments were conducted to test the rate at which O2 production was influenced by the availability of inorganic carbon. In all experiments, a varying concentration of (either 0.1%, 0.4%, 0.6%, 0.8%, or 1.0%) sodium bicarbonate was assigned to each lab bench, to use as the solution in which the aquatic plants were submerged. In the experiment my partner and I conducted, ~225 mL of distilled water was poured into two 250 mL Erlenmeyer flasks. These would later be used as photosynthetic systems— an experimental control to regulate temperature changes.

The equation that was used was molarity NaOH equals moles NaOH divided by volume NaOH in liters. The stoichiometry of the reaction of citric acid with NaOH was used to determine the moles of citric acid for

Finding the average mL NaOH added during the steep section of the curve. The mL are added together and then divided by the number of values used. Using stoichiometry to find the concentration of CH3COOH. The equation n =Cxv fis used to find the moles of NaOH, which can then be changed into moles of CH3COOH with a mole ratio The moles are converted into the concentration using C=n/V. Finding the concentration of H30+ by using initial pH of the equilibrium.

Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have enough of or too much of one ingredient , which would be defined as limiting and excess reagent, respectively.

One mole of anything equals 6.022 x 1023, also known as Avogadro’s number. The mass of one mole can be determined by Molar mass= 1

The lab manual states that for the titration of NaOH and HCl, a volume of 7mL of titrant should complete the reaction, however, the average for the experiment was only 6.25mL. This smaller amount of NaOH could have occurred by adding too much phenolphthalein, which would have caused the substance to turn pink sooner, rather than when the reaction was complete since phenolphthalein is a weak acid. Another example of error occurred in the titration of NaOH and H2SO4, a substantial difference appeared in the theoretical ratio of 2:1 and the experimental ratio of 2.5:1. This could have occurred by adding past the titration end point, resulting in more NaOH than necessary, thus altering the ratio. Both reactions involving Ba(OH)2, had relatively low percent errors, especially in the HCl reaction (approximately 5%) and a higher percent error with H2SO4 (approximately 20%).

a. Our assessments align with the Science Grade level Expectations. The standards followed for this assessment were: 7.Sci7Inquiry.1A.a Formulate testable questions and hypotheses 7.Sci7Inquiry.1A.c Design and conduct a valid experiment 7.Sci7Inquiry.1B.b Determine the appropriate tools and techniques to collect data 7.Sci7Inquiry.1B.c Use a variety of tools and equipment to gather data (e.g., microscopes, thermometers, analog and digital meters, computers, spring scales, balances, metric rulers, graduated cylinders, stopwatches) 7.Sci7Inquiry.1C.a Use quantitative and qualitative data as support for reasonable explanations (conclusions) 7.Sci7Inquiry.1D.a Communicate the procedures and results of investigations and explanations through: oral presentations, drawings and maps, data tables (allowing for the recording and analysis of data relevant to the experiment, such as independent and dependent variables, multiple trials, beginning and ending times or temperatures, derived quantities), graphs (bar, single line, pictograph),equations and writings Based on these standards, the learning goal for this unit is, “the student will be able to design valid experiments,” and the learning target is, “I can conduct valid experiments.” Lessons taught prior to this assessment were used to prepare students for this unit assessment, the benchmark assessment, and will become the

Next, the other error that might happen is the filter funnel is not inserted properly into the mouth of the conical flask causing some of the hydrochloric acid to be evaporated in the form of vapours. As some of the hydrochloric acid is evaporated, the concentration of the hydrochloric acid will be affected which will lead to the inaccuracy of the

Imagine having 20 pieces of bread and 10 pieces of ham. How many ham sandwiches can be made? This question is exactly what this topic is about. The world wants to know ‘’how much,” whether it is chemistry or daily activities in life, this question is answered by Stoichiometry.