Complete combustion of $0.858 \mathrm{~g}$ of compound $X$ gives $2.64 \mathrm{~g}$ of $\mathrm{CO}_2$ and $1.26 \mathrm{~g}_{\text {of }} \mathrm{H}_2 \mathrm{O}$. The lowest molecular mass $X$ can have :

JEE CHEMISTRY MCQ: SOME BASIC CONCEPTS OF CHEMISTRY

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Complete combustion of

0.858 \mathrm{~g}

of compound

X

gives

2.64 \mathrm{~g}

\mathrm{CO}_2

and

1.26 \mathrm{~g}_{\text {of }} \mathrm{H}_2 \mathrm{O}

. The lowest molecular mass

X

can have :

View answer and explanation

Correct option: A

43 \mathrm{~g}

Option B (21) is correct because it is the equivalent weight calculated based on the change in oxidation state of iron.

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{H_2}O.

mol\,\,k{g^{ - 1}})

2.24 {~L}

{CH}_4

{CO}_2

0.5 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4

0.5 \mathrm{~g}

\mathrm{Cu}(\mathrm{II})