(C) The equivalent weight is calculated using the formula: $\text{Equivalent weight} = \frac{\text{Atomic weight}}{\text{n-factor}}$.The reaction is:

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(C) The equivalent weight is calculated using the formula: $\text{Equivalent weight} = \frac{\text{Atomic weight}}{\text{n-factor}}$.The reaction is: $Fe^{2+} \to Fe^{3+} + e^-$.Here,the number of electrons lost ($n$-factor) is $1$.Therefore,$\text{Equivalent weight} = \frac{\text{Atomic weight}}{1} = \text{Atomic weight}$.

Class 11 Chemistry Some Basic Concepts of Chemistry Atomic, Molecular and Equivalent masses

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In a reaction,the ferrous $(Fe^{2+})$ ion is oxidized to ferric $(Fe^{3+})$ ion. The equivalent weight of the ion in the above reaction is equal to:

A
Half of the atomic weight
B
$1/5$ of the atomic weight
C
The atomic weight
D
Twice the atomic weight

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Some Basic Concepts of Chemistry

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Atomic, Molecular and Equivalent masses

Calculate the mass of one atom of oxygen.

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The equivalent mass of a certain bivalent metal is $20$. The molecular mass of its anhydrous chloride is

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$0.1$ mol of the following given antiviral compound $(P)$ will weigh $......... \times 10^{-1} \ g$
$Given :$ molar mass in $g \ mol^{-1} H: 1, C: 12, N: 14, O: 16, F: 19, I: 127$

DifficultJEE MAIN 2025

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Calculate the mass of a single atom of hydrogen.

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The oxide of a metal has the molecular formula $M_2O_3$. If the equivalent mass of the metal is $9$,what is the molecular mass of the oxide?

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In a reaction,the ferrous $(Fe^{2+})$ ion is oxidized to ferric $(Fe^{3+})$ ion. The equivalent weight of the ion in the above reaction is equal to:

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