The molar mass of an organic compound is 58 g/mol. 24 g of this is dissolved in 600 g water, calculate its boiling point when vapour pressure of water becomes 760 mm. `K_b" of "H_2O" is 0.513 K kg mol"^(-1)`.

Options

A. `99.371^(@)C`
B. `100.354^(@)C`
C. `102.07^(@)C`
D. `98.37^(@)C`

Answer

B

Explanation

b.p.t of `H_(2)O= 100^(@)C`
Given, `w_("organic compound") = 24g, W_(H_(2)O) = 60g, m_("organic compound")=58`
Also, `Delta T_(b)= (1000 xx K_(b) xx W)/(W xx m)= (1000 xx 0.513 xx 24)/(600 xx 58)= 0.354`
`therefore` b.pt of solution `=100+0.354= 100.354^(@)C`