When `2.56` gram of an elements is dissolved in `100` gram of carbon disulphide, boiling point is elevated by `0.24^(o)C`. Find out atomicity of the element. Boiling point of `CS_(2)` is `46^(o)C` and its heat of vaporization is `84` calorie/gram.(Atomic mass of the element `=31.98`)

When 1 mole of a solute is dissolved in 1 kg of H_(2)O , boiling point of solution was found to be 100.5^(@) C. K_(b) for H_(2)O is :

The boiling point of a solution of 5g of sulphur in 100g of carbon disulphide is 0.474^(@)C above that of pure solvent. Determine the molecular formula of sulphur in this solvent. The boiling point of pure carbon disulphide is 47^(@)C and its heat of vaporisation is 84 calories per gram.

0.65 g naphthalene (C_(10)H_(8)) was dissolved in 100 g methyl acetate. Elevation in boiling point of methyl acetate solution was 0.103^(@)C . If boiling point of pure methyl acetate is 57^(@)C , its molar heat of vaporisation will be:

When 10.6 g of a non volatile substance is dissolved in 750 g of ether, its boiling point is raised 0.266^(@)C . The molecular weight of the substance is (Given : Molal boiling point constant for ether is 2.0^(@)Ckg//mol ) Report your answer by rounding it up to nearest whole number.

0.90g of a non-electrolyte was dissolved in 90 g of benzene. This raised the boiling point of benzene by 0.25^(@)C . If the molecular mass of the non-electrolyte is 100.0 g mol^(-1) , calculate the molar elevation constant for benzene.

Calculate the boiling point of a solution containing 0.61 g of benzoic acid in 50 g of carbon disulphide assuming 84% dimerization of the acid. The boiling point and K_(b) of CS_(2) are 46.2^(@)C and 2.3 kg mol^(-1) .

In 100 g naphthalene 2.56 g sulphur is added boiling point of solution (solid) decreases by 0.68^(@)C , atomicity of sulphur is ( K_(f) of naphthalene=6.8 Km^(-1) )

The freezing point of nitrobenzene is 3^(@)C . When 1.2 g of chloroform (mol. Wt. =120) is dissolved in 100 g of nitrobenzene, freezing point will be 2.3^(@)C . When 0.6 g of acetic acid is dissolved in 100 g of nitrobenzene, freezing point of solution is 2.64^(@)C . If the formula of acetic acid is (CH_(2)O)_(n) , find the value of n.

2.56 g of suphur in 100 g of CS_(2) has depression in freezing point of 0.010^(@)C , K_(f)=0.1^(@)C (molal)^(-1) . Hence atomicity of sulphur in the solution is

When 2.56 g of sulphur was dissolved in 100 g of CS_(2) , the freezing point lowered by 0.383 K. Calculate the formula of sulphur (S_(x)) . ( K_(f) for CS_(2) = 3.83 K kg mol^(-1) , Atomic mass of sulphur = 32g mol^(-1) ]