Latent heat of fusion of ice is `1436.3 cal mol^(-1)`. Calculate the molal depression constant of water.

What do you mean by depression in freezing point of a solution ? How will you calculate the molecular mass of solute from depression in freezing point ? A solution containing 34.2 g cane sugar (C_12 H_22 O_11) dissolved in 500 g of water froze at - 0.374^@C . Calculate the freezing point depression constant of water.

When 1.3 g of a solute is dissolvedf in 169 g of water the boiling point of the solution is 100.025^@C at one atmospheric pressure. If K_b of water is 0.52 K kg mol^(-1) . Calculate the molecular mass of the solute.

The molar conductivity of 0.025 mol L^(-1) methanoic acid is 46.1 S cm^(2) "mol^(-1) . Calculate its degree of dissociation and dissociation constant. Given, lambda^(@) ( H^(+)) = 349.6S cm^(2) "mol"^(-1) and lambda^(@) ( HCOO^(-)) = 54.6 S cm^(2) "mol"^(-1)

The heat of combustion of C_10H_8(s) at constant volume is -5133kJ mol_-1 at 298K. Calculate the value of enthalpy change. (R=8.314 JK_-1 mol_-1)

Latent heat of fusion of lead is 5"cal"/(gm) and its melting point is 328^@C .How much heat is required to melt 5 gm of lead initially at 18^@C ? (Specific heat of lead = 0.031"cal"//(gm)//^@C) .

The standard free energy change for a reaction is -212.3 kJ mol_-1 . If the enthalpy of the reaction is 216.7 kJ mol_-1 , calculate the change in entropy in the reaction at 298K.

A solution of 1.25 g of a non-electrolyte in 20 g of water freezing at 271.9K with its molal depression constant , then the molecular wt. of the solute is: