A pure compound contains 2.4 g of C, 1.2 × 1023 atoms of H, 0.2 moles of oxygen atoms. Its empirical formula is

Question

A pure compound contains 2.4 g of C, 1.2 × 1023 atoms of H, 0.2 moles of oxygen atoms. Its empirical formula is (A) C 2 HO (B) C 2 H 2 O 2 (C) CH 2 O (D) CHO

Tardigrade Admin · Accepted Answer

Number of moles of C =(2.4/12)=0.2 Number of moles of H =(1.2 × 10/6.0 × 10)=0.2 Number of moles of O =0.2 mol Empirical formula is CHO.

Q. A pure compound contains $2.4 g$ of $C$ , $1.2 \times 1 0^{23}$ atoms of $H, 0.2$ moles of oxygen atoms. Its empirical formula is

$C_{2} H O$

$C_{2} H_{2} O_{2}$

$C H_{2} O$

$C H O$

Number of moles of $C = \frac{2.4}{12} = 0.2$
Number of moles of $H = \frac{1.2 \times 10}{6.0 \times 10} = 0.2$
Number of moles of $O = 0.2 m o l$
Empirical formula is $C H O$ .

Q. A pure compound contains 2.4g of C, 1.2×1023 atoms of H,0.2 moles of oxygen atoms. Its empirical formula is

C2​HO

C2​H2​O2​

CH2​O

CHO