If 0.219 g of a solute is dissolved into 7.832 g of t-butanol (normal freezing point is 25C), and the solution freezes at 26.4C, what is the molar mass of the solute in g/mole? Given kf for t-butanol = 8.3C/m. Make sure to use correct units and sig figs.

A solution is prepared disolving 2.00g of an substance in 10.0mL in water at 25°C. The freezing point of the substance is -0.350°C. Determine the molar mass of the substance. (Kf H2O=1.86°C) (Density H2O=0.9970g/mL)

1-A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)A sample of pure t-butyl alcohol weighing 6.22 g was found to have a freezing point of 24.7 °C. When 0.543 g of an unknown compound X was added to the t-butyl alcohol, the mixture had a freezing point of 21.3 °C. Calculate the molar mass of compound X. (Kf = 12.8 °C/molal for t-butyl alcohol.)   2-What is the rate law expression for the reaction A + B → C, based on the following data

What is the freezing point (in K) of a solution made by dissolving 19.543g of CCl4 in 130.0 g of benzene? Pure benzene has a freezing point of 5.5°C and a Kf = 5.12 °C/m.

Lauryl alcohol is obtained from coconut oil and is used to make detergents. A solution containin 2.50 g of lauryl alcohol in 100.0g of cyclohexane freezes at 3.75oC. the freezing point of pure cyclohexane is 6.50oC and its Kf= 20.5oC/m. Calculate the molar mass of lauryl alcohol.

A compound contains 42.9%C,2.4%H,16.6%N, and 38.1%O by mass. The addition of 3.16 g of this compound to 75 mL of cyclohexane (density is 0.779 g/mL) gives a solution with a freezing point of 0°C. The normal freezing point of cyclohexane is 6.5°C and its freezing point depression constant is 20.2°C/m. What is the empirical mass? A. 84 g/mol B. 88 g/mol C. 36 g/mol D. 55 g/mol E. 98 g/mol F. 44 g/mol

A solution contains 1.75 g of a non–volatile, non–electrolyte solute dissolved in 23.47g stearic acid.  The freezing point of the solution is 67.2⁰C.  The freezing point of pure stearic acid is 69.3⁰C and its freezing point constant, Kfp, is 4.5⁰C kg/mol.  What is the molar mass of the solute

5 L山 When 1.06 g of a certain molecular compound X are dissolved in 85.0 g of dibenzyl ether ((C,H,CH,),0), the freezing point of the solution is measured to be 0.9°C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 1 significant digit. 自 OL Check Save For Later Submit Assignment O2022 McGraw Hill LLC. AlI Rights Reserved. Terms of Use Privacy Center Accessibility EPIC 中Xe MacBook Pro F2 F3 F4 F7 F8 F10 6-5 #3 3. 2 $ 一 8 dele R. A C. W alt alt option 10 command option 1Q15

A 0.751-g sample of protein is dissolved in 50.0 mL of solution, and the solution exhibits an osmotic pressure of 4.1 torr at 25oC. Calculate the molar mass of protein. (R = 0.08206 L.atm/(mol.K); 1 atm = 760 torr; assume the protein is nonelectrolyte)

The freezing point of a liquid will change when a solute is added. Explain how the addition of salt impacts the boiling point of water. Calculate the freezing point change for a given concentration. Given that water’s freezing point is 0.00ºC and the freezing point depression constant (Kf) is 1.86 ºC･kg/mol, calculate the freezing point depression for a 4.35 molal solution (moles/kg) of NaCl in water. Assume ideal behavior of the ions.