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.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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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