The normal (at 760 mmHg, or 1 atm) boling point of water is 100°C. What mass (g. 3 sig. figs) of glucose (CH2O) would you have to dissolve in 1000 g of water to decrease the vapor pressure at 100°C to 7524 mmHg? Assume that water follows Raoult's law. MH,O) 18.02 g/mol M(CH20-1802 g/mol Answer What is the normal boiling point of the solution in the previous question? (C 4 sig. figs) Assume ideal behavior. The ebulioscopic (boiling point elevation) constant of water is K-0512 kg/mol Answer

1.   What mass of ethylene glycol (C2H6O2, molar mass = 62.1 g/mol), the main component of antifreeze, must be added to 8.5 L water to produce a solution for use in a car’s radiator that freezes at -10.0oF (-23.3oC)? Assume the density of water is exactly 1.0 g/mL. Kf of water = 1.86 oC–kg/mol Molar mass  of ethylene glycol = 62.1 g/mole

As a scuba diver descends under water, the pressure increases. At a total air pressure of 2.69 atm and a temperature of 25.0 °C, what is the solubility of N2 in a diver's blood? [Use the value of the Henry's law constant k calculated in Part A, 6.26 x 10-4 mol/(L· atm).JAssume that the composition of the air in the tank is the same as on land and that all of the dissolved nitrogen remains in the blood. Express your answer with the appropriate units.

What is the freezing point of a solution made by dissolving 45.0 g of glucose (C2H12O6) in 500. g of water? The freezing point depression constant, Kf, of water is 1.86 °C/m and the molar mass of glucose is 180.0 g/mol.   ΔTf = Kf m i   a. -0.465°C   b. -0.620°C   c. -1.86°C   d. -0.930°C

9.)  Using the data below (tabulated at 25 °C), what is the vapor pressure, in kilopascals (kPa), of a solution formed by mixing 5.37 mol of iodomethane (CH3I) with 4.27 mol of trichloromethane (CHCl3) at 25 °C? Assume ideal behavior. Substance Vapor Pressure (kPa) Iodomethane 53.9 Trichloromethane 26.2

Balance the given reaction for step 5 (use 1 for single species - even though it is not needed, please) and state the physical state of the compounds: ) + Na2SO4( ---> BaCl2( ) + BaSO4( NaCl(

The vapor pressure of diethyl ether (ether) is 463.57 mm Hg at 25°C. How many grams of aspirin, C9HsO4, a nonvolatile, nonelectrolyte (MW = 180.1 g/mol), must be added to 218.9 grams of diethyl ether to reduce the vapor pressure to 456.11 mm Hg? diethyl ether = CH3CH₂OCH₂CH3 = 74.12 g/mol. Mass= Submit Answer Retry Entire Group No more group attempts remain

EJ0.939 M What is the vapor pressure of a 45.0 % solution of glucose, CH,,06, at a particular temperature, 12 6' given that the vapor pressure of pure water at that temperature is 486 mm Hg? 186 m m Ha

The volume of HCI is 100 mL, mass of solid added is 1.008 g, Calculate moles of solid