On complete combustion 1.0 g of an organic compound (X) gave 1.46 g of ( $\mathrm{CO}}_{2}) and 0.567 g of (\mathrm{H}$ }_{2} $\mathrm{O}$ ). The empirical formula mass of compound (( $\mathrm{X})$ ) is ________ g.
(Given molar mass in ( $\mathrm{g} \mathrm{mol}^{-1} \mathrm{C}$ : 12, $\mathrm{H}$ : 1, $\mathrm{O}$ : 16))

Question

On complete combustion 1.0 g of an organic compound (X) gave 1.46 g of (

\mathrm{CO}}_{2}) and 0.567 g of (\mathrm{H}

}_{2}

\mathrm{O}

). The empirical formula mass of compound ((

\mathrm{X})

) is ________ g.
(Given molar mass in (

\mathrm{g} \mathrm{mol}^{-1} \mathrm{C}

: 12,

\mathrm{H}

: 1,

\mathrm{O}

: 16))

Quantrex Academy · Accepted Answer

Correct answer: A. 30

Moles of ' C ' (= n_ CO_2 =(1.46)/(44)= 0.033) Moles of ' C ' (= W_ C = 0.033 × 12) Moles of 'H' (=2 × n_ H_2 O = 2 × (0.567)/(18)= 0.063) Mass of ' H ' =0.0063 Mass of Oxygen ((O)= 1-(W_ c +W_ H )) (=1-(0.033 × 12+0.063 × 1)=0.541 gm) Moles of ' O ' (=(0.541)/(16)= 0.033) Empirical formula (= CH _ 2 O ) Empirical formula mass =30 .

On complete combustion 1.0 g of an organic compound (X) gave 1.46 g...

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