ipl-logo

Collecting Gas Lab Report

506 Words3 Pages

By conducting the Collecting Gas lab, it was determined that we had an actual yield of 0.0031 moles of H2 compared to a theoretical yield of 0.0030 moles of H2. By plugging in the actual and theoretical yield into the percent error formula, it was determined that there was a +3.33% error. In order to come to the conclusion of the +3.333% error, students had to complete a series of calculations. These calculations included:
Converting the recorded room temperature from Celsius to Kelvin in order to plug the temperature value into the the ideal gas equation (PV = nRT).
Converting the recorded room pressure from inches Hg to millimeters Hg in order to find the total pressure to plug into Pressure Conversion and Adjustment equation, which finds the pressure of H2. (** use the water vapor pressure chart in order to find the pressure of water) …show more content…

Calculating the theoretical yield of moles of H2 , which was used to find the percent error.
Calculating the actual yield of moles of H2 by using the ideal gas equation (PV = nRT), where P stands for pressure in mmHg, V stands for volume in Liters, n stands for the number of moles, R stands for the Gas Laws Constant (62.4 L∙mmHg/ mol∙K ), and T stands for temperature in Kelvin. Once the number of moles are solved for, the number was used to find the percent error.
Calculating the percent error by plugging in the actual yield and theoretical yield into the following

Show More
Related
631 Words | 3 Pages

In this lab there were five different stations. For the first station we had to determine an unknown mass and the percent difference. To find the unknown mass we set up the equation Fleft*dleft = Fright*dright. We then substituted in the values (26.05 N * 41cm = 34cm * x N) and solved for Fright to get (320.5g). To determine the percent difference we used the formula Abs[((Value 1 - Value 2) / average of 1 & 2) * 100], substituted the values (Abs[((320.5 - 315.8) /

Read More
1067 Words | 5 Pages

This was done by taking the absolute value of the difference between the experimental value and the actual value, dividing by the actual value and multiplying by a 100. ((87.5005-92.09382)/92.09382)

Read More
728 Words | 3 Pages

The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.

Read More
723 Words | 3 Pages

With following the procedure, the experiment was completed very easily. The technique used worked very well. The graduated cylinder were dried after each trial to ensure each water level was equal. The air bubble were risen to the top to ensure the equal amount was measured. Systematic errors can not be eliminated by averaging In principle, they can always be eliminated by changing the way in which the experiment was done.

Read More
848 Words | 4 Pages

37.8 °C and 36.3 °C 30-40 °C 3. 41.7 °C and 40.2 ° C 40-50 °C 4. 50 °C and 48 ° C 50-60 °C Average temperatures: (37.8+36.3)/2=37.05 °C (41.7+40.2)/2=40.95 °C (50+48)/2=49 °C Table 1 -The values of experiment Temperature (°C) Density (kg/m3) 26.5 995 37.05 992.5 40.95 991 49 990 70 984.856 80 982.524 90 980.272 100 977.93 Table 2. The values in steam table Temperature (°C) Density (kg/m3)

Read More
1390 Words | 6 Pages

Determining the Molar Volume of a Gas Lab Report The purpose of the experiment is to determine the molar volume of hydrogen gas at standard pressure and temperature. Excess hydrochloric acid was placed in a eudiometer and decanted with deionized water. A piece of magnesium ribbon was trapped in a copper wire cage in the eudiometer in order to keep it in place as the more dense hydrochloric acid diffused downward in the inverted eudiometer.

Read More
448 Words | 2 Pages

Both the mass of benzoic acid and the mass of benzaldehyde have a mass error of ±0.01g, therefore, to calculate the percent error is by, ((0.01g/5.68g)+(0.01g/5.78g))×100%, equaling 0.3% error for the result. Converting the percent of percent yield to percent yield, the formula is the calculated percent error of the result divided by 100%, multiplied by the percentage yield. Therefore, 98.3%×((0.3%)/(100%)), equals to 0.2%, as demonstrated in Table 2.1, thus the final answer for the percent yield of benzoic acid is 98.2%±0.2%

Read More
803 Words | 4 Pages

Also, accurate measurements was also an issue in this experiment. Using poor measuring techniques is the reason why there were two recreated solutions in Figure 6. The second recreation attempt was measured with a burette, which did improve accuracy of the solution somewhat. With the errors of this experiment now in mind, improvements in equipment sanitation, measuring techniques, and an improved knowledge of the calculations could be utilized to improve future research

Read More
630 Words | 3 Pages

In this experiment, preparative gas chromatography was performed to isolate components present in a mixture before infrared spectroscopy was utilized to determine the separated parts. At the start of the lab, unknown # C-2 at 170C was provided for testing. When the GC was ran, the retention time for fraction 1 started with 2.12 minutes and ended with 2.96 minutes. The retention time for fraction 2 started at 4.56 minutes and ended at 5.96 minutes. After centrifugation, a small amount of the sample was pulled to the bottom of the conical vials to be used in the infrared spectroscopy.

Read More
1724 Words | 7 Pages

For this experiment, Cu(s), went through many reactions with a series of reagents to produce four different copper containing compounds before being restored back to its original metallic form. The observations from each reaction were then used to determine the type of reaction it was, and various equations associated with each reaction type. The amount of copper measured at the beginning and end of the experiment were compared to one another to determine its percent recovery by using Equation 1. The percent recovery was then related back to the Law of Conservation of Mass to see if the experiment supported the law. One thing that could be changed with this experiment would be to have a proper way to decan the liquids since some of the precipitate

Read More
478 Words | 2 Pages

The water percent is determined to be 42.06%. To find a percent error, a theoretical percent water must be used. To find the theoretical percent error divide the mass of water by the mass of magnesium sulfate heptahydrate and multiply by 100 to get a percent. The theoretical percent water is

Read More
542 Words | 3 Pages

The lab performed was to test how different types of chemicals would affect rocks of similar sizes to measure the amount of mass lost due to weathering. The chemicals used for this experiment were solutions such as 50% vinegar, 10% vinegar, soda water, and regular tap water, which were used as a control. Using these samples, this experiment was conducted to showcase how different chemicals weather soil and minerals, along with how this weathering affects the topography of our environment. In order to understand the effects of chemical weathering in this experiment, it should be known that it occurs when a chemical substance such as acetic acid is introduced into an environment, causing the accelerated deterioration of soil and minerals found within the layers of the earth.

Read More
724 Words | 3 Pages

So this meant that the second formula was the actual yield. There is evidence for a pattern in chemical activity. The theoretical yields of all four problems have Sodium, but problems #1,#3,#4 have a lighter mass than equation #2. In addition the ones with more mass have a higher yield than the ones with less overall; this is because the gases in each theoretical yield are different. So this means that the mass of the gases in each yield differentiates between which one is the actual yield, and which one is

Read More
1052 Words | 5 Pages

The mass of vinegar used during the experiment was 4.108 grams. It was determined that there were .003129 moles of CH3COOH in the vinegar sample. Using this information and the molar mass of CH3COOH, which was 60.05 g/mol, the mass of acetic acid in the vinegar was calculated: 4.Vinegar is a 5% aqueous solution of acetic acid. Since the mass of acetic acid within the vinegar was calculated as .18789 g in step 3, the percent of CH3COOH was calculated using the following equation: To calculate the percent error, the experimental value of 4.5% acetic acid in vinegar was subtracted by the theoretical value of 5% and divided by 5% to yield a percent error of 8.54%. The following is a copy of the calculations done using decimals: 5.The equivalence point of the titration curve measured in step 1 was 25.25 mL of NaOH.

Read More
1545 Words | 7 Pages

INTRODUCTION A gas chromatograph (GC) can be utilized to analyze the contents of a sample quantitatively or in certain circumstances also qualitatively. In the case of preparative chromatography, a pure compound can be extracted from a mixture. The principle of gas chromatography can be explained as following: A micro syringe is used to inject a known volume of vaporous or liquid analyte into the head or entrance of a column whereby a stream of an inert gas acts a carrier (mobile phase). The column acts as a separator of individual or chemically similar components.

Read More

More about Collecting Gas Lab Report

Related Topics

Open Document