Emperical Formula
Chemistry
Level
2
A compound has 24.74% of Carbon, 2.062% of Hydrogen, 24.74% of Oxygen, 16.495% of Sulphur and 31.96% of Phosphorous. Find the Molecular formula if the Vapour density of that compound is 388 g/cc.
None of the above
C4H4O3SP2
C14H14O16S2P4
C16H16O12S4P8
C18H18O6S6P4
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1 solution
The solution for this is C16H16O12S4P8. Of course this is hypothetical. If we solve by using the steps : 1) Divide the respective percentages with their respective atomic masses. 2) After getting the figures from step 1, divide those figures with the least value obtained from al those figures from step 1. 3) The finally obtained values must be in their integral form not in decimals, if they are then a) either is they are very close to end or start i.e. 0.98 or 0.01. Then round it. b) or else multiply all finally obtained values with a suitable integer to get an integer. 4) This is the simplest ratio. Combinning we get Emperical formula 5) Take the Emperical formula weight and keep it aside. 6) Molecular mass = 2 * Vapour Density, Substitute and find out molecular mass. 7) Molecular formula = (Emperical formula)n (...read as taken n times...) where n = (Molecular formula weight)/(Emperical formula weight) 8) calculate 'n' and find it out. substitute in formula of step 7. 9) Got it !