1. Demonstrate the Law of Multiple Proportions with the following data: a. Iron forms two compounds with chlorine, compound X and compound Y. When 3.00 g of compound X was analyzed, it was found that 1.68 g of Cl combined with 1.32 g of Fe. When 5.00 g of compound Y was analyzed, it was found that 3.28 g of Cl combined with 1.72 g of Fe. To illustrate the Law, one needs to know how much of one element combines with the same mass as the other element in each compound, but the data above give different masses for both Fe and Cl. One way to standardize the data is to find out how much of one element, say C1, combines with exactly 1 g of the other, say Fe. This can be done by a simple proportion method ("if 1.75 g of Cl combines with 1.25 g of Fe, how many g of Cl would combine with 1.00 g of Fe...") Do this for both compounds, X and Y.
1. Demonstrate the Law of Multiple Proportions with the following data: a. Iron forms two compounds with chlorine, compound X and compound Y. When 3.00 g of compound X was analyzed, it was found that 1.68 g of Cl combined with 1.32 g of Fe. When 5.00 g of compound Y was analyzed, it was found that 3.28 g of Cl combined with 1.72 g of Fe. To illustrate the Law, one needs to know how much of one element combines with the same mass as the other element in each compound, but the data above give different masses for both Fe and Cl. One way to standardize the data is to find out how much of one element, say C1, combines with exactly 1 g of the other, say Fe. This can be done by a simple proportion method ("if 1.75 g of Cl combines with 1.25 g of Fe, how many g of Cl would combine with 1.00 g of Fe...") Do this for both compounds, X and Y.
Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Mark S. Cracolice, Ed Peters
Chapter6: Chemical Nomenclature
Section: Chapter Questions
Problem 3E: Write the chemical formula of each of the following: a The compound made up of a crystal with one...
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1. Demonstrate the Law of Multiple Proportions with the following data:
a. Iron forms two compounds with chlorine, compound X and compound Y. When 3.00 g of compound X was analyzed, it was found that 1.68 g of Cl combined with 1.32 g of Fe. When 5.00 g of compound Y was analyzed, it was found that 3.28 g of Cl combined with 1.72 g of Fe.
To illustrate the Law, one needs to know how much of one element combines with the same mass as the other element in each compound, but the data above give different masses for both Fe and Cl. One way to standardize the data is to find out how much of one element, say C1, combines with exactly 1 g of the other, say Fe. This can be done by a simple proportion method ("if 1.75 g of Cl combines with 1.25 g of Fe, how many g of Cl would combine with 1.00 g of Fe...") Do this for both compounds, X and Y.
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