Iodine (I) and fluorine (F) form a series of binary compounds with the following compositions:Compound Mass % I Mass % F1 86.979 13.0212 69.007 30.9933 57.191 42.8094 48.829 51.171(a) Compute in each case the mass of fluorine that combines with 1.0000 g iodine.(b) By figuring out small whole-number ratios among thefour answers in part (a), show that these compoundssatisfy the law of multiple proportions.
Iodine (I) and fluorine (F) form a series of binary compounds with the following compositions:Compound Mass % I Mass % F1 86.979 13.0212 69.007 30.9933 57.191 42.8094 48.829 51.171(a) Compute in each case the mass of fluorine that combines with 1.0000 g iodine.(b) By figuring out small whole-number ratios among thefour answers in part (a), show that these compoundssatisfy the law of multiple proportions.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter2: Chemical Compounds
Section: Chapter Questions
Problem 143QRT: The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry...
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Iodine (I) and fluorine (F) form a series of binary compounds with the following compositions:
Compound Mass % I Mass % F
1 86.979 13.021
2 69.007 30.993
3 57.191 42.809
4 48.829 51.171
(a) Compute in each case the mass of fluorine that combines with 1.0000 g iodine.
(b) By figuring out small whole-number ratios among the
four answers in part (a), show that these compounds
satisfy the law of multiple proportions.
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