Stearic acid, `C_17H_35COOH`, has a density of `0.85g//cm^3`. The molecule occupies an area of `0.205nm^2` in a closed packed surface film. Calculate the length of the molecule. (Molecular weight of Stearic acid is 284.48gm/mole)

0.6 mL of acetic acid (CH_3COOH) , having density 1.06g mL^-1 , is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was 0.0205^@C . Calculate the van't Hoff factor and the dissociation constant of acid

At 25^(@)C and at a certain pressure, 3.7 g of a gas occupies the same volume as the volume occupied by 0.184 of H_(2) gas at 17^(@)C and the same pressure. Calculate molar mass of the gas.

When C_2H_5OH and CH_3-COOH are mixed in equivalent proportion, equilibrium is reached when 2/3 of acid and alcohol are used. How much ester will be present when 2g molecules of acid were to react with 2g molecule of alcohol ?

Combustion of 0.2 of a monobasic organic acid produces 0.505 g CO_(2) and 0.0892g H_(2)O . 0.183g of the above acid requires 15 cm^(3) of (N/10) NaOH solution for complete neutralisation. Determine the molecular formula of the organic acid.

The well know mineral flourite is chemically calcium fluoride. It is a well known fact that in one unit cell of this mineral, there are four Ca^(2+) ions and eight F^(-) ions and Ca^(2+) ions are arranged in f.c.c. lattice. The F^(-) ions fill all the tetrahedral holes in the face centred cubic lattice of Ca^(2+) ions. The edge length of the unit cell is 5.46xx10^(-8) cm. The density of the solid is 3.18"g cm"^(-3) . Use this information to calculate Avogadro's number (Molar mass of CaF_(2)=78.0"g mol"^(-1) )

The densities of water and water vapour are 1.0 g*cm^(-3) and 0.0006g*cm^(-3) respectively at 100^(@)C and 1 atmm pressure. At this temperature, the total volume occupied by watrer molecules in 1L of water vapour is-

The mole fraction of a solute in a binary solution is 0.1. At 298 K, molarity of this solution is same as its molality. Density of this solution at 298 K is 2.0 g cm^(-3) . The ratio of molecular weights of the solute and the solvent (M_("solute")//M_("solvent")) is

0.93g of a compound containing C, H and N, on buring produces 2.64g CO_(2) and 0.63g H_(2)O . In another experiment, 0.186g of that compound yield 24.62cm^(3) of nitrogen at 1 atmospheric pressure at 27^(@)C . Molecular weight of the compound is 93. what is its molecular formula?