The number of hydrogen atoms present in `25.6 g` of sucrose `(C_12 H_22 O_11)` which has a molar mass of `342.3g` is :

Calculate mass of 2.7moles of C_(12)H_(22)O_(11) (molar mass = 342 g/ mol)

An aqueous solution of sucrose ( C_(12)H_(22)O_(11) ) having a concentration of 34.2gram/ litre has an osmotic pressure of 2.38 atmospheres at 17^(@) C. For an aqurous solution of glucose ( C_(6)H_(12)O_(6) ) to be isotonic with this solution , its concentration should be :

Calculate number of neutrons present in 12 xx 10^25 atoms of oxygen (8O^17) : (Given : N_A=6 xx 10^23 )

The osmotic pressures of 0.010 M solutions of KI and sucrose ( C_(12)H_(22)O_(11) ) are 0.432 atm and 0.24 atm respectively. The van't Hoff factor for KI is :

Calculate the molecular mass of C12H22O11

Calculate the osmotic pressure of a solution containing 10 gram each of glucose (C_6H_12O_8) and sucrose (C_12H_22O_11) in 1000cm^3 of the soluton at 25^@C . (R=0.083 L bar K^-1 mol^-1)

Calculate the weight of CO having the same number of oxygen atoms as are present in 22 g of CO2 .

An aqueous solution containing 6 g of ureas in 500 mL of solution has a density equal to 1.05. if the molar mass of urea is 60. then the molality of solution is

What is the density of wet air with 75% relative humidity at 1 atm and 300 K? Given : vapour pressure of H_(2)O is 30 torr and average molar mass of air is 29 g mol^(_1) .

An aqueous solution of glucose is made by dissolving 10 g of glucose (C_6H_12O_6) in 90 g of water at 303 K. if the vapour pressure of pure water at 303 K be 32.8 mm Hg, what would be the vapour pressure of the solution?