On dissolving 19.5g `CH_2F` COOH in 500g of water, a depression of `1^@C` in freezing point of water is observed. Calculate the vant Hoff factor and dissociation constant of Fluoroacetic acid. `(Given, K_f = 1.86 K kg mol^-1)`

Calculate the freezing point of an aqueous solution containing 10.50g of MgBr_2 = 184g, K_f for water = 1.86 K kg mol^-1 .

Calculate the charge in coulombs required for oxidation of 2 moles of water to oxygen. (Given 1 F = 96500 mol^-1 )

A 0.561 m solution of an unknown electrolyte depresses the freezing point of water by 2.93^@C . What is Vant Hoff factor for this electrolyte? The freezing point depression constant (K_f) for water is 1.86^@C Kg mol^-1 .

A solution of sucrose (molecular mass 342 u) is prepared by dissolving 0.84 g in 100g of water at 298K. Calculate the freezing point of water in the solution. (K_f for water = 1.86 K kg mol^-1)

Calculate the amount of NaCl which must be added to one kilogram of water so that the freezing point of water is depressed by 3K (Given K_f = 1.86KKg mol^(-1) )

0.5g KCl was dissolved in 100g water and the solution originally at 20^@C , freeze at -0.24^@C . Calculate the percentage ionization of salt, K_f for per 1000g of water = 1.86K .

A solution of sucrose (molecular mass 342 u) is prepared by dissolving 0.84 g in 100g of water at 298K. Calculate the boiling point of water in the solution (K_b for water = 0.52 K kg mol^-1)

A 0.1539 molal aqueous solution of canesugar (molar mass = 342g mol^-1) has a freezing point 271K. While the freezing point of pure water is 273.15k. What will be the freezing point of an aqueous solution, containing 5g of glucose (Mol mass = 180g mol^-1) per 100g of solution?

The rate constants of a reaction at 500K and 700K are 0.02s^-1 and 0.07s^-1 respectively. Calculate value of activation energy for the reaction. (Given R = 8.314 JK^-1 mol^-1)

Calculate the depression in the freezing point of water when 10 g of CH_3CH_2CHClCOOH is added to 250 g of water. K_a = 1.4xx10^-3 , K_f = 1.86 K kg mol^-1 .