What is the osmotic pressure (in atm) of a 1.36M aqueous solution of urea [(NH2)2CO] at...
What is the osmotic pressure of 0.250 M aqueous urea (CON2H4) at 25 °C. R = 0.08206 L atm/mol K and R = 8.3145 J/K mol)
What is the osmotic pressure (atm) of an aqueous solution with a volume of 0.750 L that contains 5.0 g of methanol, CH3OH, at 37∘C? Round the answer to two significant figures.
The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH4NCO(aq)->(NH2)2CO(aq) is second order in NHANCO with a rate constant of 1.10x10-2 M-min-7. If the initial concentration of NHANCO is 0.451 M, the concentration of NHANCO will be 6.00x10-2 M after minutes have passed. Submit Answer Retry Entire Group 8 more group attempts remaining
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What is the concentration of a 500 mL urea [(NH2)2CO] solution containing 0.820 moles of urea? A. 0.00164 M B. 1.6 M oC 610 M D. 0.610 M
Urea, (NH2)2CO, which is widely used in fertilizers and plastics, is quite soluble in water. If you dissolve 6.51 g of urea in 15.0 mL of water, what is the vapor pressure of the solution at 24 °C? Assume the density of water is 1.00 g/mL. The vapor pressure of water at 24 °C is 22.4 mmHg. mmHg
1.a)The average osmotic pressure of sea water is 30 atm (atmospheres). Calculate the concentration of urea (CH4ON2) at 25 ° C that exerts the same pressure as seawater. R = 0.082 atm L/ mol K 1.b) There is a 1M solution of CH3COOH (acetic acid) in a total volume of 450 mL. What is the molality (m) of the solution? (ρ solution = 1.15 g / mL).
1.) A 0.046 M aqueous solution of FeCl, has an osmotic pressure of 4.09 atm at 28°C. a. Calculate the percentage difference of the van't Hoff factor from the ideal value. b. What should be the concentration of this aqueous solution if this is in ideal condition?
A dilute aqueous CaCl2 solution at 25 degrees celsius has an osmotic pressure pi = 10bar. What is the vapor pressure(in bar units) above the solution? The density of water at 25 degrees Celsius is water (25 degrees Celsius) = 0.997gmL.
How many grams of urea, (NH2)2CO (the product of protein metabolism in animals) must be dissolved in 146.3 g of H2O to cause a freezing point depression of 1.996 degrees celsius? Kf=1.86 C/m
The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein’s molar mass. The solution contained 3.50-g of protein dissolved in sufficient water to form 5.00-L of solution. The osmotic pressure of the solution at 25oC was found to be 1.54-mmHg. (Hint: Remember to convert mmHg to atm) Calculate the molar mass of the protein.