An aqueous magnesium chloride solution having a density of 1.049 g/cm3 is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution boils.
An aqueous magnesium chloride solution having a density of 1.049 g/cm3 is found to have an...
A solution is prepared from 4.5743 g of magnesium chloride and 43.246 g of water. The vapor pressure of water above this solution is found to be 0.3630 atm at 348.0 K. The vapor pressure of pure water at this temperature is 0.3804 atm. Find the value of the van't Hoff factor i for magnesium chloride in this solution.
A aqueous dextrose solution having a density of 1.04g/mL freezes at -1.15 C. Find the osmotic pressure of this solution at 25 degree C.
3.) An aqueous solution of Alz(S04), has a freezing point temperature of -7.8585 °C and an osmotic pressure of 46.71 atm. Calculate the density of the solution in g/ml. Assume ideal operating condition at 25 °C.
A 36.5% by mass of C6H12O6, aqueous solution is prepared in the lab. the density of the solution is 2.97 g/ml. what is the osmotic pressure of the solution at 42 OC ( R=0.08206 L*atm/mol*K)
A solution is prepared from 4.5728 gg of magnesium chloride and 43.236 gg of water. The vapour pressure of water above this solution is found to be 0.3630 barbar at 348.0 KK. The vapour pressure of pure water at this temperature is 0.3804 barbar. Find the value of the van't Hoff factor (ii) for magnesium chloride in this solution.
1. 1200 mL aqueous solution of 45 g of ethylene glycol and 80 g of sucrose were prepared with a density of 1.37 g/mL. Assume that the solution behaves ideally. Notes: The vapor pressures of water and ethylene glycol at 20 °C are 17.54 torr and 0.06 torr, respectively, and Kb and Kf of water are 0.51 K/m and 1.86 K/m, at 25 °C respectively. a. What is the freezing point of this solution? b. What is the vapor pressure,...
an aqueous solution is 4.30m lithium chloride. the density of the solution is 1.127 g/mL calculate a) molarity b) mole fraction c) percent by mass
A sample of an unknown gas is found to have a density of 1.53 g/L at a pressure of 0.612 atm and a temperature of 48 °C. Assume ideal behavior. The molar mass of the unknown gas is ? g/mol.
2. The density of iron at 910 °C is 7.571 g/cm3 for the a-form and 7.633 g/cm3 for the y-form. The heat absorbed in the α-γ transition is 912 J/mole. (Note that I cm2 atm. = 0.1013 J.) Disregarding the dependency of change in volume with pressure, what is the change in molar volume of iron (in cm/mole)? Calculate the equilibrium temperature for this transformation at a pressure of 1000 atm a. b.
A sample of an unknown gas is found to have a density of 2.53 g/L at a pressure of 1.04 atm and a temperature of 49 °C. Assume ideal behavior. The molar mass of the unknown gas is ___________g/mol.