DateHourNamewere measured before the experiment began and the data is shown below.The iron was left to react with the oxygen in a glass beaker. The mass of the iron and beaker2. A student performed an experiment to determine how much rust (Fe,0,) could be producesexperimentally if a certain mass of iron was allowed to completely react with excess Oxygen.Quantity MeasuredBeakerMassa. Balance the chemical equation20.32 g25.09 gFe +_02→ Fe,0,Fe,O3Beaker and FeMass of Feb. Calculate the amount of Fe,O, that should be produced if all of the Iron reacts.At the end of the experiment the student found the mass of the beaker and the Fe,Oz and addedthe following column to his data table.Quantity MeasuredBeaker and Fe2O3Massc. What is the experimental mass of Fe,O3?27.18 gd. Calculate the Percent Yield of Fe203 and show your work below.V1

The reaction given is, => Fe + O2 → Fe2O3

Date Hour were measured before the experiment began and the data is shown below. The iron was left to react with the oxygen in a glass beaker. The mass of the iron and beake 2. A student performed an experiment to determine how much rust (Fe,0) could be produce experimentally if a certain mass of iron was allowed to completely react with excess oxgen. Mass a. Balance the chemical equation Quantity Measured Beaker 20.32 g 25.09 g Fe + Fe,O Beaker and Fe Mass of Fe b. Calculate the amount of Fe,O, that should be produced if all of the Iron reacts. At the end of the experiment the student found the mass of the beaker and the Fe,O, and added the following column to his data table. Quantity Measured Beaker and Fe2O3 Mass c. What is the experimental mass of Fe,0,? 27.18 g d. Calculate the Percent Yield of Fe,0, and show your work below

Date Hour were measured before the experiment began and the data is shown below. The iron was left to react with the oxygen in a glass beaker. The mass of the iron and beake 2. A student performed an experiment to determine how much rust (Fe,0) could be produce experimentally if a certain mass of iron was allowed to completely react with excess oxgen. Mass a. Balance the chemical equation Quantity Measured Beaker 20.32 g 25.09 g Fe + Fe,O Beaker and Fe Mass of Fe b. Calculate the amount of Fe,O, that should be produced if all of the Iron reacts. At the end of the experiment the student found the mass of the beaker and the Fe,O, and added the following column to his data table. Quantity Measured Beaker and Fe2O3 Mass c. What is the experimental mass of Fe,0,? 27.18 g d. Calculate the Percent Yield of Fe,0, and show your work below

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter8: Chemical Reactions

Section: Chapter Questions

Problem 1E: Consider the following particulate-level representation of a chemical equation: The white spheres...

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