LYLLISINLASH Homework 2 chp 13 Question 25 of 28 (1 point) Question Attempt: 1 of Unlimited...
A certain substance X has a normal freezing point of 6.8 C and a molal freezing point depression constant Kf=7.51C kg x mol-1 . A solution is prepared by dissolving some urea ((NH2)2CO) in 600 of X. This solution freezes at 5.0 C . Calculate the mass of urea that was dissolved. Be sure your answer has the correct number of significant digits.
8. The normal freezing point of a certain liquid X is 0.7 °C, but when 15. g of urea, (NH2)2CO, are dissolved in 250. g of X, it is found that the solution freezes at -5.8 °C instead. Use this information to calculate the molal freezing point depression constant Kr of X. Be sure your answer has the correct number of significant digits.
The normal freezing point of a certain liquid X is 4.1 C , but when 27.84 g of urea ((NH2)2CO) are dissolved in 750 g of X , it is found that the solution freezes at -0.7 C instead. Use this information to calculate the molal freezing point depression constant Kf of X . Be sure your answer has the correct number of significant digits
A certain liquid X has a normal freezing point of 5.50 °C and a freezing point depression constant K =4.39 °C-kgmol. A solution is prepared by dissolving some urea (CH4N20) in 800. g of X. This solution freezes at 3.6 °C. Calculate the mass of CH4N20 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. x 6 ?
= 1.89 °C kg.mol. Calculate the boiling point of A certain substance X has a normal boiling point of 108.2 °C and a molal boiling point elevation constant K a solution made of 45. g of urea ((NH2), CO) dissolved in 700. g of X. Be sure your answer has the correct number of significant digits. 1°C x 6 ?
the solution freezes at The normal freezing point of a certain liquid X is - 2.80 °C, but when 22. g of benzamide (C,H,NO) are dissolved in 200. g of - 7.4 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Round your answer to 2 significant digits. *, - more 09
A certain substance X melts at a temperature of -9.9 °C. But if a 250. g sample of X is prepared with 9.10 g of urea ((NH) CO dissolved in it, the sam is found to have a melting point of -12.0 °C instead. Calculate the molal freezing point depression constant K, of X. Be sure your answer has the correct number of significant digits. [°C mol'.kg x 5 ? Save For Later Sult Check
The normal freezing point of a certain liquid X is 6.60 °C, but when 27. g of potassium bromide (KBr) are dissolved in 300. g of X the solution freezes at 4.9 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Be sure your answer is rounded to the correct number of significiant digits. Ķ, = 0 °C kg x s ?
Part A:
Part B:
The normal freezing point of a certain liquid X is – 8.1 °C, but when 7.9 g of urea ((NH),CO) are dissolved in 650, 8 of X, it is found that the solution freezes at -9.7 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Be sure your answer has the correct number of significant digits. c mol 1 .kg X ? Consider the following data on some weak...
QUESTION 25 The molar mass of a compound can be determined by the freezing point depression method. The solution must be relatively dilute and you must know the molal freezing point depression constant of the solvent, Kf: Which statement regarding Kris true? Kf should be small so that the solvent will not sublimate, Kf will change depending on what solute is dissolved in the solvent. Kfshould be negative so the freezing point of the solution will decrease. Kfshould be large...