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 & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter2: Atoms Molecules And Ions
Section2.8: Instrumental Analysis: Determining Compound Formulas
Problem 3.4ACP: Given that the density of argon is 1.78 g/L under standard conditions of temperature and pressure,...
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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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