Home
Class 12
CHEMISTRY
Assuming the formation of an ideal solut...

Assuming the formation of an ideal solution, determine the boiling point of `a` mixture containing `1560g` benzene (molar mass `=78`) and `1125g` chlorobenzene (molar mass `=112.5`) using the following against an external pressure of `1000` Torr.

Promotional Banner

Similar Questions

Explore conceptually related problems

The following is a table of the vapour pressure of pure benzene and chlorobenzene. Determine the boiling point of a mixture containing 40 mole percent of benzene and 60 mole percent of chlorobenzene at a pressure of 1000 mm Hg.

What is the mass percentage of each component in a mixture containing 22 g of methanol in 112g of benzene?

The molarity of solution containing 15.20 g of urea, (molar mass = 60) dissolved in 150 g of water is

The molarity of solution containing 15.20 g of urea, (molar mass = 60) dissolved in 150 g of water is

The boiling of a solution containing 1.5 g of dichlorobenzene in 100 g of benzene was higher by 0.268^(@)C . Calculate the molar mass of dichlorobenzene ( k_(b) for benzene 2.62 degree/molal)

The boiling point of a solution containing 1.5 g of a dichlorobenzene in 100 g of benzene was higher by 0.268^@C . Calculate the molar mass of dichlorobenzene (K_b for benzene=2.62 degree molal^(-1)) .

The boiling point of a solution containing 1.5 g of dichlorobenzene in 100 g of benzene was higher by 0.268^@C . Calculate the molar mass of dichlorobenzene. K_b forbenzene = 2.42 K kg mol^-1