Find the mass of urea (CH4N2O) needed to prepare 51.3 g of a solution in water in which the mole fraction of urea is 7.53×10−2.
Find the mass of urea (CH4N2O) needed to prepare 51.3 g of a solution in water...
Find the mass of urea (CH4N2O) needed to prepare 51.3 g of a solution in water in which the mole fraction of urea is 7.66×10−2.
7. What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 46% urea by mass? 8. What volume of a 0.850 M solution of CaCl2 contains 1.28 g of solute? 9. The volume of a 27.0% (by mass) solution is 162.9 mL. The density of the solution is 1.128 g/mL. What is the mass of solute in this solution? 10. Concentrated sodium hydroxide is 19.4 M and has a density of 1.54 g/mL. What is the...
what is the mole fraction of urea, CH4N2O, in an aqueous solution that is 59% urea by mass?
The vapor pressure of an aqueous solution of urea, CH4N2O, is 291.2 mm Hg. The vapor pressure of water at this temperature is 355.1 mm Hg. Calculate the mole fraction of urea in this solution. a. 0.180 b. 0.220 c. 0.500 d. 0.820 e. 1.22 please show all work
The industrially important chemical, urea [CH4N2O; molar mass = 60.0 grams per mole], is prepared from the reaction of ammonia [NH3: molar mass = 17.0 grams per mole] with carbon dioxide [CO2; molar mass = 44.0 grams per mole] according to the following: 2 NH3 + CO2 CH4N2O + H2O If one reacts 132.0 grams of CO2 with 136.0 grams of ammonia, which of these would be the limiting reagent?
What mass of water must be used to prepare a solution of 25.5 g of CaCl2 dissolved in water if the mole fraction of the CaCl2 in solution is 0.105?
When 23.7g of urea (CH4N2O) are dissolved in 750. g of a certain mystery liquid X, the freezing point of the solution is 7.20°C less than the freezing point of pure X. Calculate the mass of potassium bromide that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i = 1.62 for potassium bromide in X. Be sure your answer has a unit symbol, if necessary, and round your answer to...
How much urea (CH4N2O; molecular weight: 60.056 g/mol) in grams do I need to add to 1L water to have a final concentration of 20 mg/L Total Nitrogen as Nitrogen or TN-N. Nitrogen molecular weight is 14.0067 g/mol.
0. 000 45) The concentration of urea in a solution prepared by dissolving 16 g of urea in 20 g of H2O is _% by mass. The molar mass of urea is 60.0 g/mol. A) 0.48 B) 0.44 C) 80 D) 0.80 E) 44 46) The concentration of a benzene solution prepared by mixing 11.0 g C6H6 with 38.0 g CCl4 is molal. A) 2.40 B) 3.71 C) 0.622 D) 0.508 E) 0.289 47) The mole fraction of He in...
a solution was prepared by dissolving 27.0 g KOH in 100 g water. A) what is mole fraction of KOH in solution? B) what is mass percent?C) what is the molality? 2. A solution was prepared by dissolving 27.0 g KOH(s)in 100.0 g water. You may use the chart below if you find usefiul to answer questions a) -e) MW (g/mol Mass ()moles 56.1 H20 18.0 Solution (a) What is the mole fraction of KOH in the solution? (5 pts...