How many grams of manganese(II) iodide (308.7 g/mol), must be dissolved in 258.0 grams of water to raise the boiling point by 0.500°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula K, ("C/m) Ke(°C/m) Water Ethanol H,O CH;CH,OH CHCI; 0.512 1.86 1.22 1.99 Chloroform 3.67 2.53 5.12 CGH5 Diethyl ether CH;CH,OCH,CH; Benzene 2.02 g manganese(II) iodide.

How many grams of manganese(II) iodide (308.7 g/mol), must be dissolved in 258.0 grams of water to raise the boiling point by 0.500°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula K, ("C/m) Ke(°C/m) Water Ethanol H,O CH;CH,OH CHCI; 0.512 1.86 1.22 1.99 Chloroform 3.67 2.53 5.12 CGH5 Diethyl ether CH;CH,OCH,CH; Benzene 2.02 g manganese(II) iodide.

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...

See similar textbooks

Similar questions

how do I calculate the boiling point of methanol if its boiling point is 72.2 degrees Celsius , the molar boiling point elevation constant foe methanol is 2.7 degrees per m What is the boiling point of a solution prepared by dissolving 50g of acidic acid in 100g of methanol?(boiling point for the solvent =94.7 degrees Celsius)
The normal boiling point of a certain liquid X is 91.9 °C, but when 86.4 g of urea ((NH₂), CO) are dissolved in 850. g of X, it is found that the solution boils at 94.0 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. C-mol¹-kg 0.2 X
The normal boiling point of a certain liquid X is 124.9 °C, but when 31. g of urea ((NH,) CO) are dissolved in 350. g of X, it is found that the solution boils at 127.0 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. 9. Round your answer to 2 significant digits. - 1 |°C• mol •kg
Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is soluble in benzene, C6H6. At 25 °C, the vapor pressure of pure benzene is 100.84 torr. What is the vapor pressure of a solution made from dissolving 19.9 g of biphenyl in 25.8 g of benzene? (anwser needs to be in torr)
A certain liquid x has a normal freezing point of 1.30 °C and a freezing point depression constant K,- 3.30 °C-kg'mol!. A solution is prepared by dissolving some glycine (c,H,NO,) in 850. g of x. This solution freezes at - 2.2 °C. Calculate the mass of c,H,NO, that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. ?
What is the freezing point of a solution that is made by dissolving 68.7 grams of the nonelectrolyte ethanol, C,H,0, in 1000 grams of water? freezing point = °C
when 7.94 g of xylene was added to 132.5 g of cyclohexane, the freezing point of the solution was -4.9 C. what is the molar mass of xylene?
The normal boiling point of a certain liquid X is 128.10 °C, but when 35.3 g of urea (CH4N2O) are dissolved in 350. g of X the solution boils at 130.9 °C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. °C-kg ☐ x10 K-0 = mol 5
The freezing point of water H,0 is 0.00°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in water is antifreeze (ethylene glycol). If 13.20 grams of antifreeze, CH,OHCH,OH (62.10 g/mol), are dissolved in 245.3 grams of water.. The molality of the solution is m. The freezing point of the solution is °C. Submit Answer Retry Entire Group 9 more group attempts remaining sited Cengage Learning | Cengage Technical Support 100%
Consider following aqueous solutions:2.75 m sucrose / 1.50 m NaC1 / 1.00 m LiPO4 / Pure Water / 1.25 m MgCl2Which solution has the highest boiling point?Which solution has the highest freezing point?Which solution has the lowest vapor pressure?
please explain