A solution contains 25% H2O , 25% C2H5OH and 50% CH3COOH by mass .The mole fraction of H2O would be :
0.25
2.5
0.502
5.03
C.
0.502
Mole fraction of H2O =
Let the total mass of solution = 100 g
Mass of H2O = 25 g
Mass of C2H5OH = 25g
Mass of CH3COOH = 50 g
Moles of H2O = = 1.388
( Molar mass of H2O = 18)
Moles of C2H5OH = = 0.543
( Molar mass of C2H5OH = 46)
Moles of CH3COOH = = 0.833
( Molar mass of CH3COOH = 60)
Total no. of moles = 1.388 + 0.543 + 0.833 = 2.764
Mole fraction of H2O = = 0.502
An organic substance containing carbon , hydrogen and oxygen gave the following percentage composition .
C = 40.687 % , H = 5.085% and O = 54.228 %
What is the empirical formula of the compound ?
CH3O
C2H2O
CH4O
C2H3O2
How many grams of CO2 will be produced by the complete combustion of 2 moles of ethanol ?
132 g
44 g
176 g
88 g
Which of the following changes with change in temperature ?
Mole fraction
Formality
% (w/W)
Molality
Equal weight of CO and CH4 are mixed together in an empty container at 300 K. The fraction of total pressure exerted by CH4 is.
Ksp of CaSO4.5H2O is 9 10-6, find the volume for 1 g of CaSO4 (M.wt. = 136).
2.45 litres
5.1 litres
4.52 litres
3.2 litres
Which ofthe following sequence contains atomic number of only representative elements?
55,12,48,53
13,33,54,80
3,33,53,87
22,33,55,66.
100 cm3 of a given sample of H2O2 gives 1000 cm3 of O2 at S.T.P. The given sample is
10% H2O2
90% H2O2
10 volume H2O2
100 volume H2O2