A compound has an empirical formula C 2 H 4 O. An independent analysis gave a value of 132.16 for its molecular mass. What is the correct molecular formula?

Question

A compound has an empirical formula C 2 H 4 O. An independent analysis gave a value of 132.16 for its molecular mass. What is the correct molecular formula? (A) C 4 H 4 O 5 (B) C 10 H 12 (C) C 7 O 3 (D) C 6 H 12 O 3

Tardigrade Admin · Accepted Answer

Empirical formula weight C 2 H 4 O =(12 × 2+4+16)=44 Molecular formula=( text Mol. wt / text Eq. formula wt. ) × Empirical Formula =(132.1/44) × Emperical formula =3 × C 2 H 4 O = C 6 H 12 O 3

Q. A compound has an empirical formula $C_{2} H_{4} O$ . An independent analysis gave a value of $132.16$ for its molecular mass. What is the correct molecular formula?

$C_{4} H_{4} O_{5}$

$C_{10} H_{12}$

$C_{7} O_{3}$

$C_{6} H_{12} O_{3}$

Empirical formula weight $C_{2} H_{4} O = (12 \times 2 + 4 + 16) = 44$
Molecular formula $= \frac{Mol. wt}{Eq. formula wt.} \times$ Empirical Formula
$= \frac{132.1}{44} \times$ Emperical formula
$= 3 \times C_{2} H_{4} O = C_{6} H_{12} O_{3}$

Q. A compound has an empirical formula C2​H4​O. An independent analysis gave a value of 132.16 for its molecular mass. What is the correct molecular formula?

C4​H4​O5​

C10​H12​

C7​O3​

C6​H12​O3​