A certain liquid X has a normal freezing point of – 9.40 °C and a freezing point depression constantK,=4.04 °C kg•mol1. A solution is prepared by dissolving some iron(III) chloride (FeCl,) in 150. g of X. This solutionfreezes at - 13.0 °C. Calculate the mass of FeCl, that was dissolved.Round your answer to 2 significant digits.doArCheckExplanationTerms of Use Privacy Center | Accessibility©2022 McGraw Hill LLC. All Rights Reserved.FEBtv3.

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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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A certain liquid X has a normal freezing point of – 9.40 °C and a freezing point depression constant
K,=4.04 °C kg•mol
1
. A solution is prepared by dissolving some iron(III) chloride (FeCl,) in 150. g of X. This solution
freezes at - 13.0 °C. Calculate the mass of FeCl, that was dissolved.
Round your answer to 2 significant digits.
do
Ar
Check
Explanation
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©2022 McGraw Hill LLC. All Rights Reserved.
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$Given a liquid X, Normal freezing point = - 9.40 ° C Freezing point of solution = - 13.0 ° C Depression in freezing point (∆ T_{f}) = 3.60 ° C K_{f} = 4.04 ° C Kg {mol}^{- 1} Mass of solvent = 150 \times 10^{- 3} Kg$

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