The normal boiling point of a certain liquid X is 144,50 °C, but when 46. g of iron(III) chloride (FeCl,) are dissolved in 500. g of X the solution boils at 145.4 °C instead. Use this information to calculate the molal boiling point elevation constant K of X. Round your answer to 1 significant digit. °C-kg K, = mol
The normal boiling point of a certain liquid X is 144,50 °C, but when 46. g of iron(III) chloride (FeCl,) are dissolved in 500. g of X the solution boils at 145.4 °C instead. Use this information to calculate the molal boiling point elevation constant K of X. Round your answer to 1 significant digit. °C-kg K, = mol
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter11: Solutions
Section: Chapter Questions
Problem 46P
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![The normal boiling point of a certain liquid X is 144.50 °C, but when 46. g of iron(III) chloride (FeCl,) are dissolved in 500. g of X the solution boils at
145.4 °C instead. Use this information to calculate the molal boiling point elevation constant K of X.
Round your answer to 1 significant digit.
°C-kg
K, = 0
X10
%3D
mol
Submit Assignn
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Transcribed Image Text:The normal boiling point of a certain liquid X is 144.50 °C, but when 46. g of iron(III) chloride (FeCl,) are dissolved in 500. g of X the solution boils at
145.4 °C instead. Use this information to calculate the molal boiling point elevation constant K of X.
Round your answer to 1 significant digit.
°C-kg
K, = 0
X10
%3D
mol
Submit Assignn
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27
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F5
F7
F8
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23
$4
&
4
6.
7
8
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Y
D
H.
K
alt
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option
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