benzene at a certain temperature is 0.850bar. A non- ute solid weighing 0.5 g when added...
When 8.59 g of an unknown, non-volatile, non-electrolyte, X was dissolved in 100. g of benzene, the vapor pressure of the solvent decreased from 100 torr to 97.5 torr at 299 K. Calculate the molar mass of the solute, X.
1f. At an unknown temperature a solution made of (7.740x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.51x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (5.360x10^1) g/mol. 1g. A solution is made of two volatile solutes: Chemical A (with a pure vapor pressure of 80.0 mm Hg) and Chemical B (with a pure vapor...
At an unknown temperature a solution made of (5.180x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.54x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at this unknown temperature? The molar mass of the solute is (4.620x10^1) g/mol. Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is...
1a: 19.930 g of a non-volatile solute is dissolved in 395.0 g of water. The solute does not react with water nor dissociate in solution. Assume that the resulting solution displays ideal Raoult's law behaviour. At 90°C the vapour pressure of the solution is 521.11 torr. The vapour pressure of pure water at 90°C is 525.80 torr. Calculate the molar mass of the solute (g/mol). 1b: Now suppose, instead, that 19.930 g of a volatile solute is dissolved in 395.0...
When 9.31 g of an unknown non-electrolyte is dissolved in 50.0 g of benzene, the boiling point increased by 3.16 degrees C. If the Kbp of the solvent is 2.53 K/m, calculate the molar mass of the unknown solute. The answer is 149 ± 2% looking for explanation how to work this problem
A sample of 2.00 g of the non-volatile compound urea, CO(NH2)2 (molar mass = 60 g/mol), is dissolved in 20.0 grams of water. What is the vapor pressure of water above this solution? The vapor pressure of pure water at the temperature of the experiment is 0.150 atm. a. 0.045 atm b. 0.010 atm c. 0.038 atm d. 0.146 atm e. 0.150 atm