    Question

# A gaseous compound is composed of 85.7% by mass carbon and 14.3% by mass hydrogen. Its density is 2.5 g/litre and one mole of the gas occupies 44.8 L of space at a particular temperature and pressure. Determine the molecular formula of the compound.

A
C4H4
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B
C4H8
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C
C8H16
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D
C8H8
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Solution

## The correct option is B C8H16Since we have the volume of 1 mol of gas and the density in g/L, looking at the units, the molecular mass will be given by d×V M=2.5 g L−1×44.8 L=112 g Empirical formula, Assuming 100 g of the compound, Moles of C = 85.712 Moles of H = 14.31 Their mole ratio, 85.712:14.31=7.14:14.3=1:2 ∴ Empirical Formula is CH2 So, molecular formula would be (CH2)n, where n=11212+2=8 Molecular formula is C8H16.  Suggest Corrections  0      Similar questions  Related Videos   Coordination Complexes
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