Question

A compound has a haemoglobin-like structure. It has one $Fe$. It contains $4.6 \%$ of $Fe$. The approximate molecular mass is

• A. $100 \,g \,mol ^{-1}$
• B. $1200 \,g \,mol ^{-1}$
• C. $1400 \,g \,mol ^{-1}$
• D. $1600 \,g \,mol ^{-1}$

Answer 1

Answer: (B)

$1 \,g$ -atom of Fe $(56\, g \,Fe )$ is present in $I$ mole of the compound.

As $4.6 \,g$ of $Fe$ is present in $100 \,g$ of the compound.

$\therefore 56 \,g$ of $Fe$ will be present in $\frac{100}{4.6} \times 56 \,g$

$=1217 \,g$ of the compound

Hence, approximate molecular mass $=1200 \,g \,mol ^{-1}$