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A certain liquid X has a normal freezing point of 0.40 °C and a freezing point depression constant K₁ = 5.78 °C-kg-mol. A solution is prepared by dissolving some glycine (C₂H₂NO₂) in 850. g of X. This solution freezes at −5.2 °C. Calculate the mass of C₂HNO₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits.

A certain liquid X has a normal freezing point of 0.40 °C and a freezing point depression constant K₁ = 5.78 °C-kg-mol. A solution is prepared by dissolving some glycine (C₂H₂NO₂) in 850. g of X. This solution freezes at −5.2 °C. Calculate the mass of C₂HNO₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits.

Chemistry
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
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1 A certain liquid X has a normal freezing point of 0.40 °C and a freezing point depression constant K = 5.78 °C·kg⋅mol A solution is prepared by dissolving some glycine (C₂HÃNO₂) in 850. g of X. This solution freezes at −5.2 °C. Calculate the mass of C₂H²NO₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. 1 g | x10 S
Transcribed Image Text:1 A certain liquid X has a normal freezing point of 0.40 °C and a freezing point depression constant K = 5.78 °C·kg⋅mol A solution is prepared by dissolving some glycine (C₂HÃNO₂) in 850. g of X. This solution freezes at −5.2 °C. Calculate the mass of C₂H²NO₂ that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. 1 g | x10 S
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