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20. A solution consisting of 0.378 mol of methylbenzene, C6H5CH3, in 264 g of nitrobenzene, C6H5NO2,...
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation:2NF_3(g) N_2(g) + 3F_2(g) When 1.82 mol of NF_3, is placed in a 3.00 L container and allowed to come to equilibrium at 800 K, the mixture is found to contain 0.0261 mol of N_2. What is the value of k_p, at this temperature? 398 times 10^-4 1.91 times 10^-5 1.80 times 10^-3 4.43 times 10^-7 3.87 times 10^-4 A red blood cell placed in pure water...
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.
The freezing point of nitrobenzene is 5.67∘C at 1 atmand the freezing point depression constant is 8.1∘Cm. What is the freezing point of a 0.105 m solution of a nonvolatile nonelectrolyte solute in nitrobenzene? Your answer should have two significant figures
A pure solvent freezes at 6.35 degrees Celsius and a pure solute freezes at 832.0 degrees Celsius. The molar mass of the solvent is 96.4 g/mol and the molar mass of the solute is 78.5 g/mol. The freezing point depression constant for the solvent is 6.33 degrees/m. A solution is made of 1.012 g of the solute and 15.280 g of the solvent, determine its freezing point in degrees Celsius.
2. A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). The freezing point of the solution is __________°C. The freezing point of pure ethanol is -114.6 °C at 1 atm. The molal-freezing-point-depression constant (Kf) for ethanol is 1.88 °C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively.
A solution is prepared by dissolving 5.00 g of glycerin () in 201 g of ethanol The freezing point of the solution is ________°C. The freezing point of pure ethanol is -114.6 °C at 1 atm. The molal-freezing-point-depression constant () for ethanol is 1.99 °C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively. -115.1 -119.4 0.537 -109.8 -114.1
A solution is prepared by dissolving 2.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). The freezing point of the solution is _______ degrees celsius. The freezing point of pure ethanol is -114.6 degrees celsius at 1atm. The molal-freezing point depression constant (Kf) for ethanol is 1.99 degrees celsius/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively.
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 substance used to make detergents. A solution of 5.00 g of that substance in 100. g of benzene freezes at 4.100°C. What is the molar mass of this substance? (freezing point of benzene is 5.444°C, molal freezing point depression constant of benzene is 5.12 oC/m) (Consider the # of significant figures.)