Calculate the mass of chloroform (CHCl3, an organic solvent) that contains 1.00x10^12 molecules of chloroform
A polymer of large molar mass is dissolved in the organic solvent chloroform (CHCl3) at 25 °C, and the resulting solution rises to a final height of 7.99 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 3.97 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 1.48 g cm-3.
Calculate the mass of 4.275x1021 molecules of chloroform (CHCl3). (when I take the given molecules and divide avagrados 6.022x10^23 than multiply by molar mass of 119.38g/mol I get a number way off...what am i doing wrong?).
A beaker contains 44.9 mL of chloroform (CHCl3), density is 1.48 g/mL). Determine how many molecules of chloroform are in the beaker.
A polymer of large molar mass is dissolved in the organic solvent dimethylformamide (C3H7NO) at 25 °C, and the resulting solution rises to a final height of 17.5 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 5.03 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 0.944 g cm-3. Molar mass polymer =
Calculate the Freezing point of a solution containing 0.6 kg of chloroform, CHCL3, and 42.0 g of eucalptol, C10H18O. the normal freezing point of cholorform is (-63.5 c ) and the Kf IS 4.68 c/m
The nonvolatile, nonelectrolyte aspirin, C9H8O4 (180.1 g/mol), is soluble in chloroform, CHCl3. Calculate the osmotic pressure generated when 12.0 grams of aspirin are dissolved in 179 ml of a chloroform solution at 298 K. The molarity of the sollution is? The osmotic pressure of the solution is?
Kf for chloroform is 4.68 C/m: normal freezing point go chloroform is -63.5 C. Calculate the freezing point of a solution containing 750 g of chloroform CHCL3 and 85 g of a solute that has a molar mass of 154 g/mol..
1) if 6.85 of glucose( C6H12O6, molar mass=180.2 g/mol) is dissolved in 155g of chloroform( CHCL3,molar mass= 119.4 g/mol) , what is the boiling point of the solution. ( the boiling point of pure CHCl3 is 61.2 celsius, and Kb = 3.63 celsius/m for CHCl3) 2) a,) Liquid ammonia (boiling point = -33.4C) can be used as a refrigerant and heat transfer fluid. How much energy is needed to heat 25.0 g of NH3(l) from -65.0C to -12.0C? Heat of...
2. In attempting to calculate the density of chloroform, CHCl3, Riley determines the following densities: 1.30 g/mL, 1.35 g/mL, 1.32 g/mL, 1.23 g/mL, 1.13 g/mL, and 1.39 g/mL. a. Calculate the average density of chloroform from his data. b. If the accepted density of chloroform is 1.48 g/mL, calculate the percent error. C. Was Riley's data accurate? Was the data precise? Explain your reasoning. Experiment 1: Determination of the Density of Water and nft page 14 3. For each of...
7. (4 pts) For each of the following solid organic molecules, circle the solvent that would be the best for re-crystallization. CH3 HN Н3Слл CH3 "CH3 OH HO H2N-NH2 Water Water Water Water 95% Ethanol 95% Ethanol 95% Ethanol 95% Ethanol Hexane Hexane Hexane Hexane