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...
part c calculate the freezing/boiling point for 18.0 g of decane, C10H22, in 50.0 g CHCl3 part e calculate the freezing/boiling point for 0.48 mol ethylene glycol and 0.18 mol KBr in 166g H2O Carbon w orden TABLE 13.3 · Molal Boiling-Point-Elevation and Freezing-Point-Depression Constants Normal Boiling Normal Freezing Solvent Point ("C) K. (°C/m) Point (°C) K(°C/m) Water, H2O 100.0 0.51 0.0 1.86 Benzene, CH 80.1 2.53 5.5 Ethanol, C H OH 78.4 1.22 -114.6 1.99 Carbon tetrachloride, CCI 76.8...