Kate and Landon - Lab Report (1)

pdf

School

University of Notre Dame *

*We aren’t endorsed by this school

Course

180

Subject

Chemistry

Date

Apr 3, 2024

Type

pdf

Pages

Uploaded by BailiffRiver13800

Intro : Sugar, sweet carbohydrates, are found in food produced naturally. In this lab, sugar was taken, composed of CH ₂ O (empirical formula) and burnt to try to discover its percent composition and empirical formula. By measuring the amount of water lost and carbon remaining, use that to determine the percent composition and empirical formula of sugar. In empirical formulas the lowest whole number ratio of atoms of elements in a compound. The empirical formula for H 4 O 2 would be H ₂ O. The percent composition is percent of each mass present in a compound. Gravimetric analysis in the lab is when taking the information of the mass and using it to find out the composition of the compound. In the lab, a bunsen burner was used to burn the sugar and measure the amount of water burnt off. Depending on the heat of the burner and the amount of time burned, the amount of water burnt off and carbon remaining will significantly change. After burning, assume the remaining mass left is carbon and the mass lost is purely water. If the sugar is burned, the percent composition and empirical formula will be found because only the water will burn off during the chemical reaction, leaving only the carbon. Procedure/Materials - Ring stand - Bunsen burner - Digital scale - Flint lighter - Wire mesh - Aluminum foil - Tongs

- Sugar 1. Obtain a piece of aluminum foil and wire mesh 2. Fold the aluminum foil to create a container that the sugar will be contained atop the wire mesh 3. Measure the mass of the aluminum foil container. Add 3 scoops of sugar to the aluminum foil container and measure the mass of the foil container and sugar 4. Place the setup onto a ring stand with a bunsen burner underneath. 5. Use the flint lighter to light the bunsen burner and adjust the flame. (The flame tip should be close to, but not touching the bottom of the wire mesh) 6. Continue heating the sugar until it has been completely burnt. Tongs were used to gently adjust the setup if needed for even burning. 7. Once burnt, turn off the burner. The tongs removed the aluminum foil container off the ring stand and placed gently on the table to allow time to sufficiently cool down. 8. Measured the mass of the foil and burnt sugar. 9. Disposed of the sugar and aluminum foil. Returned all materials to the original location Data Mass of Aluminum Foil 3.03 grams Mass of Aluminum Foil and Sugar 6.86 grams Mass of Aluminum Foil and Sugar Post Burn 6.41 grams The difference in mass before and after burning .45 grams

Percent Composition of Water Composition Mass Percentage Hydrogen 2.02 grams 11.2% Oxygen 16.00 grams 88.8% Water 18.02 grams 100% Hydrogen = 11.2 % Oxygen = 88.8% 2.02𝑔 18.02𝑔 16.00𝑔 18.02𝑔 Percent Composition of the mass of Hydrogen and Oxygen lost Oxygen 0.45g 88.8% · 0.4 grams lost Hydrogen 0.45 11.2% · 0.05 grams lost Percent Composition of Sugar 3.83 grams of sugar

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

3.38 grams of Carbon = 3.38𝑔 3.83𝑔 88.3% 0.4 grams of Oxygen = 0.4𝑔 3.83𝑔 10.4% 0.05 grams of Hydrogen 0.05𝑔 3.83𝑔 1.3% Empirical Formula of Sugar Grams to Mole Calculation Carbon 88.3 grams → 7.35 mol = 7.35 ?𝑜? 0.65 ?𝑜? 11.3 Oxygen 10.4 grams → 0.65 mol = 0.65?𝑜? 0.65 ?𝑜? 1 Hydrogen 1.39 grams → 1.29 mol = 1.29?𝑜? 0.65 ?𝑜? 1.98 Final Results

Empirical Formula C 11 H 2 O Percent Composition Carbon: 88.3% Hydrogen: 1.3%. Oxygen: 10.4% Discussion To calculate the mass of water (H 2 O) lost, subtracted the weight of the aluminum from the sugar, then subtracted the sugar pre burn and post burn. To calculate the percent composition, the percentage of hydrogen and oxygen composing the water, starting with the H, find the molar mass of water. From there, calculate the percentage of H using the mass of H and mass of water resulting in 11.2%. Similarly, to calculate the percentage of O, use its mass divided by the total mass of water, resulting in 88.8%. From there, use the percent composition like a ratio and multiply the mass of H 2 O by the percentage of hydrogen and oxygen. This results in .05g H and and .40g O. Assuming only the water was burned off and only the carbon remains, assume the mass of carbon is the mass remaining (3.38g). Using masses already calculated for H and O, use the masses to calculate the percent composition of the sugar. From there, calculate the empirical

formula by assuming there to be 100g of sugar then converting them to moles. From there, divide by the smallest molar mass. After, round to the nearest whole number. This results in the empirical formula of C 11 H 2 O. This is an inaccurate representation of the true empirical formula: CH 2 O. The assumption for it to be all water that was burned off is incorrect as there is too much carbon in the calculated empirical formula compared to the true one. Conclusion The purpose of this lab was to determine the empirical formula of sugar which resulted in C 11 H 2 O and the percent composition of sugar which had the result of Carbon being 88.3%, Oxygen being 10.4%, and Hydrogen being 1.3%. The percent composition of the mass can be determined through the process of gravimetric analysis where the percent composition of the water lost was obtained during the burning process of the sugar. During this lab, the substance that was provided was 3.83 grams of sugar and during the burning process there was .45 grams of water lost turning the sugar black where only carbon is remaining. Once the amount of water lost was figured out, the percent composition of the hydrogen and the oxygen was determined. And when the composition of water was revealed then, the process of finding the percent composition of the sugar itself was calculated which led to the percentages of carbon making up 88.3% of the sugar, oxygen making up 10.4% and Hydrogen 1.3%. When the percentage composition of the sugar was figured out, that data then was used to get the empirical formula of C 11 H 2 0. The experimental error that could have occurred was that the sugar was not fully burned with only carbon remaining. This could have been possible as the sugar post-burn was still a dark brown, not black. If the substance was still a dark brown color, then the remaining mass (assumed to be carbon) will be larger than the true result and there will be less mass (assumed to

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

be water)loss during the burning process. If the sugar was burnt for longer into the black color then the empirical formula could have been calculated more accurately as the amount of carbon would have decreased exponentially. Another experimental error that occurred was assuming all remaining mass of sugar was pure carbon. This is not true and will alter the calculations of the empirical formula. In the future when performing the lab, the sugar should be burned for longer and should not assume that the mass remaining is only carbon. In pharmacies, gravimetric analysis may be used to measure the precise amount of active ingredient needed to prepare a medication accurately. Gravimetric analysis records changes in mass. In pharmacies, known masses of a compound/ingredient are weighed and then transferred to a container. The material is then heated and evaporated. Then, the vaporized material is collected and weighed. This allows the mass of the original sample to be calculated. Gravimetric analysis may be used to watch the purity and consistency of drug products in the production process (Jordi Labs). For example, when manufacturing a pill/medication, gravimetric analysis can measure the amount of each active ingredient that must be integrated to ensure the quality and efficacy of medication. Therefore, gravimetric analysis has many uses in pharmaceutical sciences by heating then measuring masses of compounds and ensuring consistency in medication. References “Gravimetric Analysis: Analyte: Mass Measurement: Supplier.” Jordi Labs , https://jordilabs.com/lab-testing/technique/bench-chemistry/gravimetric-analysis/

Related Documents

Lab 1.docx

Life Chemistry Data Collection (Exp.4).pdf

Chapter 6 Quiz _ Nutrition for Health Sciences 33523-933.pdf

Anthrax FBI Case.docx

CE150 HW Assignment 7.pdf

Lab Assignment 9.docx

AC1803_asgt3_W_2023 2.pdf

Experiment 8.docx

Microwave Assisted Esterification.docx

Experiment 7-Oxidation Puzzle .docx

Homework 4_ Nuclear and Wind Energy_ EGEE 101 (SP24 WC ONLINE MERGED).pdf

Lesson 27.1 Participation_ Introduction to Biomass_ EGEE 101 (SP24 WC ONLINE MERGED).pdf

Recommended textbooks for you

Introductory Chemistry: A Foundation

Chemistry

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:Cengage Learning

World of Chemistry, 3rd edition

Chemistry

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Brooks / Cole / Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Cengage Learning

SEE MORE TEXTBOOKS

Recommended textbooks for you

Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning