What would be the molar mas of a compound if 6.21 g of it dissolved in 24.0 g of chloroform a solution that has a boiling point of `68.04^(@)C`? Given that the boiling point of pure chloroform is `61.7^(@)C` and `K_(b) for chloroform= 3.63^(@)C/m`.

What would be the molar mass of a compound if 6.21g of it dissolved in 24.0 g of chloroform form a solution that has a higher boiling point of 68.04^@C and the boiling point of pure chloroform is 61.7^C and the boiling point elevation constant K_b for chloroform is 3.63^@C/m .

What would be the molar mass of a compound if I 6.21 g of it dissolved in 24 .0 g of chloroform form a solution that has a bolling point of 68.04""^(@)C. The bolling point of pure chloroform is 61.7^(@)C and the boiling point elevation constant, K_(b) for chloroform is 3.63^(@) C/m.

(a) Differentiate between molarity and molality in a solution. What is the effect of temperature change on molarity and molality in a solution? . (b) What would be the molar mass of a compound if 6.21 g of it dissolved in 24.0g of chloroform from a solution tharhas a boiling point of 68.04^@C . The boiling point of pure chloroform is 61.7^@C and the boiling point elevation constant, K_b for chloroform is 3.63^@C//m .

(a) Differentiate between molarity and molality in a solution. What is the effect of temperature change on molarity and molality in a solution? . (b) What would be the molar mass of a compound if 6.21 g of it dissolved in 24.0g of chloroform from a solution tharhas a boiling point of 68.04^@C . The boiling point of pure chloroform is 61.7^@C and the boiling point elevation constant, K_b for chloroform is 3.63^@C//m .

The enthalpy of vaporization of chloroform is 29.4 kJmol^(-1) at its normal boiling point of 61.7^(@) C. What is the entropy of condensation of chlorofom at this temperature?

The enthalpy of vaporization of chloroform is 29.4 kJmol^(-1) at its normal boiling point of 61.7^(@) C. What is the entropy of condensation of chlorofom at this temperature?