The molal freezing point depression constant K,-2.44 °C.kg mol for a certain X, the solution freezes at -9.6 °C. calculate the freezing point of pure X Round your answer to 2 significant digits.
A certain substance X −6.5°C =Kf·7.48°C·kgmol−1 NH22CO 850.g X −12.9°C
Round your answer to
2
significant digits.
The molal freezing point depression constant K,-2.44 °C.kg mol for a certain X, the solution freezes...
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 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.
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
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 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 ?
= 4.47 °C-kg-mol. Calculate the freezing point of a A certain liquid X has a normal freezing point of 4.20 °C and a freezing point depression constant K solution made of 22.g of potassium bromide (KBr) dissolved in 550. g of X. Round you answer to 2 significant digits. 3°C X 5 ?
1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf = 0.777°C/m. What is the predicted freezing point (in °C) of a solution made from this solvent that is (1.90x10^0) m in a non-electrolyte solute? 1i. When (8.23x10^1) g of a non-electrolyte is dissolved in (5.2600x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the...
A certain liquid X has a normal freezing point of 7.80 °C and a freezing point depression constant K,=3.03 °C kg mol. Calculate the freezing point of a solution made of 15.6g of urea (CH N,0) dissolved in 200. g of X. Be sure your answer is rounded to the correct number of significant digits. O°C
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 ?
ADVANCED MATERIAL Using the Kland Kb equations with electrolytes A certain liquid X has a normal freezing point of 2.60 °C and a freezing point depression constant k, = 5.29 °C kg-mol . A solution is prepared by dissolving some ammonium chloride (NHCl) in 800. g of X. This solution freezes at 0.9 °C. Calculate the mass of NHCl that was dissolved. Round your answer to 2 significant digits. Explanation Check