Ethanol (C2H6O) is used as an additive in gasoline . Calculate the molality of an ethanol solution prepared by dissolving 78.6 g of ethanol in enough water to produce 225 g of solution .
Select one:
A. 11.67 m
B. 7.59 m
C. 349.33 m
D. 0.349 m
E. 0.537 m
Ethanol (C2H6O) is used as an additive in gasoline . Calculate the molality of an ethanol...
Cadmium bromide is used in photography and lithography. Calculate the molality of a solution prepared In dissolving 50.65 g of CdBr_2 in 285.0 g of water. 0.030.35 m 0.6529 0.4446 m none these choices is The solubility of nitrogen gas at 35 degree C and a nitrogen pressure of 0.756 atm is what is the value of the Henry's Law constant in mol L^-1 atm^-1?
What is the concentration of NO3-ions in a solution prepared by dissolving 20.0 g of Ca(NO3)2 in enough water to produce 300 mL of solution? 0.406 M 0.537 M 0.813 M. O 0.203 M
Calculate the molality of a dextrose (mw = 180.16 g/mole) solution prepared by dissolving 52.8 g dextrose in 500 mL of water (density of the solution is 1.06).
A solution was prepared by dissolving 37.0 g of KCl in 225 g of water. Calculate the mole fraction of the ionic species KCl in the solution. Calculate the molarity of KCl in the solution if the total volume of the solution is 239 mL. Calculate the molality of KCl in the solution.
3. The density of a 4.53 M NH, solution is 0.9651 g/mL Calculate the molality 4. Calculate the freezing and boiling points of a solution made by mixing 10.5 g magnesium iodide with 150.0 g water. 5. A solution prepared by dissolving 0.56 g of a non-ionic solute in 25.0 g benzene freezes at 4.45°C. What is the molar mass of the solute?
(4 Points) Gasoline is primarily a mixture of hydrocarbons and is sold with an octane rating that is based on a comparison with the properties of isooctane (CsHis), which has an enthalpy of vaporization of 35.8 kJ/mol and a normal boiling point of 98.2 °C. Determine the vapor pressure of isooctane on a very hot day when the temperature is 38.0 °C. 1. (4 Points) A 15.0 mg sample of a protein was dissolved in water to produce 5.00 mL...
8. A solution is prepared by dissolving 0.434 moles of ethanol, C2H60, in 150. grams of water. Calculate the molality of the solution, freezing point of the solution, and boiling point of the solution. (Kf of H2O 1.86°C/m; fp of H20 = 0.00°C; Kb of H20 = 0.512°C/m; BP of H20 100.00°C)
Calculate the mole fractions of ethanol, C_2 H_5 OH (1), and water in an alcohol and water solution, prepared by dissolving 50.0 g of ethanol in 250.0 grams of water.
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
How do you find the mass percent, mole fraction, and the
molality for these two problems?
P1. (Sec. 11.1) A solution is prepared by dissolving 113 grams of acetone (C3H6O) in 662 grams of water. With this information, calculate the solution's mass percent % of the solute, mole fraction of the solute, and the solutions molality. a) b) c) d) e) Mass Percent: 88.7%; Mole Fraction (Solute): 0.9068; & Molality: 5.70 mol/kg Mass Percent: 11.3%; Mole Fraction (Solute): 0.0932; &...