Question

i want to know how to work out the problem

1.)Calculate the molarity of a solution made by 20.2 g of sucrose, C12H22O11, in enough water tomake 650 mL of solution. The molar mass of sucrose is 342 g/mol.  

2.) A solution was made by mixing 39.5 g of carbon disulfide (CS2, MW= 76.15g/mol), and 24.3 gof acetone (CH3OCH3, MW = 58.08g/mol). Assuming ideal solution behavior, calculate thetotal vapor pressure above the solution at 35 °C, given that the vapor pressure of carbondisulfide and acetone are 515 torr and 332 torr, respectively.

The experimentally measuredtotal pressure for this solution was found to be 643 torr. Is this solution ideal? If not, what typeof deviation did this solution display? (6 points)

First calculate the mole fraction of each component of the solution.

Then use Raoult’s law to calculate the partial vapor pressures for carbon disulfide and acetone.

Then calculate the total pressure by adding both partial pressures.

3.)Butylated hydroxytoluene (BHT) is used as an antioxidant in processed food. A solution of5.00 g of BHT in 200.0 g of benzene had a freezing point of 4.880 ºC. What is the molecularweight of BHT?

4.) An aqueous solution of sulfuric acid is made by dissolving 585.0 g of sulfuric acid in enoughdistilled water to make a one liter solution. Calculate the molarity, the molality the mass% andthe mole fraction of sulfuric acid in this solution. The density of this solution is 1.350 g/mL.MW H2SO4 = 98.00 g/mol

Answer 1