A solution is prepared by dissolving 2.00 g of glycerin (C3H8O3) in 201 g of ethanol...
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.
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A solution is prepared by dissolving 2.00 g of glycerin (C3H8O3)
in 201 g of ethanol...
2. A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3) in 201 g of...
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...
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
9. 65) A soltion is prepared by dissolving 7.00 g of gycerin (C3Hg03) in 201 g...
9. 65) A soltion is prepared by dissolving 7.00 g of gycerin (C3Hg03) in 201 g of ethanol (C2HsOH). The freezing point of the solution isoC freezing-point-depression constant (Kp for ethanol is 1.99°C/m. The molar °C. The feezing point of pure ethanol is -114.6°C at 1 atm. The molal- masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol respectively.
The vapor pressure of a solution containing 38.7 g glycerin (C3H8O3) in 146.2 g ethanol (C2H5OH)...
The vapor pressure of a solution containing 38.7 g glycerin (C3H8O3) in 146.2 g ethanol (C2H5OH) is 40.4 torr and 20 degrees C. Calculate the vapor pressure of pure ethanol at 20 degrees C assuming that glycerin is a nonvolatile, nonelectrolyte solute in ethanol. Vapor pressure = _________ torr
Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/m...
Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86°C/m and Kb = 0.512°C/m. A) -3.33°C B) 0.887°C C) -1.65°C D) 3.33°C E) 0.654°C
Suppose a solution of 0.615 g of glycerol is dissolved in 10.0 g of ethanol. Upon...
Suppose a solution of 0.615 g of glycerol is dissolved in 10.0 g of ethanol. Upon testing, you determined the new freezing point for the mixture to be -115.9 °C. If the normal freezing point of pure ethanol is-114.6 °C and its freezing point depression constant (K) equals 1.99 C/m, what is the molar mass of glycerol?
Benzaldehyde ( MM = 106.18 g/mol) also known as oil of almonds is used in the...
Benzaldehyde ( MM = 106.18 g/mol) also known as oil of almonds is used in the manufracture of dyes and perfume and in flavorings. what would be the freezing point of a solution prepared by dissolving 106.345 g of benzaldehyde in 1.687 kg of ethanol? kf=1.99, freezing point of pure ethanol = -117.3 degree Celsius a) moles of benzaldehyde b) kg of ethanol c) molality d) freezing point depression : delta Tf= kf×m e) freezing point of the solution
The literature value for the freezing point of C2H5OH is -114.6 °C. The Kf for this...
The literature value for the freezing point of C2H5OH is -114.6 °C. The Kf for this solution is 2.00 °C/m. Calculate the freezing point (in °C) of a solution that is formulated by dissolving 50.0 g of C3H8O3 (a non-electrolyte) into 200.0 g of C2H5OH.
What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of in 115 g of water? [Use these Molar Mass...
What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of in 115 g of water? [Use these Molar Masses: Ca = 40, N = 14, O = 16. Also, the molal freezing point depression constant for water is 1.86 °C/m.]
1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point...
1.0345 g of palmitic acid dissolved in 8.7545 g of stearic acid. Calculate the freezing point of the solution. The molar mass of palmitic acid is 256.48 g/ mol. The molal freezing point constant , Kf for stearic acid is 4.5 degrees C/ m and pure stearic acid freezes at 69.3 degrees Celsius.
9. 65) A soltion is prepared by dissolving 7.00 g of gycerin (C3Hg03) in 201 g of ethanol (C2HsOH). The freezing point of the solution isoC freezing-point-depression constant (Kp for ethanol is 1.99°C/m. The molar °C. The feezing point of pure ethanol is -114.6°C at 1 atm. The molal- masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol respectively.
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