(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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Class 11

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Some Basic Concepts of Chemistry

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Atomic, Molecular and Equivalent masses

The atomic mass of noble gases is determined by which of the following relationships?

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What should be the equivalent weight of phosphorous acid,if $P=31, O=16, H=1$?

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In nature,carbon exists as a mixture of $C^{12}$ and $C^{13}$. The average atomic mass of carbon is $12.011$. What is the percentage abundance of $C^{12}$ in nature?

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$0.16 \ g$ of dibasic acid required $25 \ mL$ of decinormal $NaOH$ solution for complete neutralization. The molecular weight of the acid will be:

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The ratio of the mass of '$x$' atoms of an element to the mass of '$x$' carbon atoms is $9:1$. Find the molar mass of the element if the molar mass of carbon is $12 \text{ g/mol}$. (in $\text{ g/mol}$)

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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:

Similar Questions

The atomic mass of noble gases is determined by which of the following relationships?

What should be the equivalent weight of phosphorous acid,if $P=31, O=16, H=1$?

In nature,carbon exists as a mixture of $C^{12}$ and $C^{13}$. The average atomic mass of carbon is $12.011$. What is the percentage abundance of $C^{12}$ in nature?

$0.16 \ g$ of dibasic acid required $25 \ mL$ of decinormal $NaOH$ solution for complete neutralization. The molecular weight of the acid will be:

The ratio of the mass of '$x$' atoms of an element to the mass of '$x$' carbon atoms is $9:1$. Find the molar mass of the element if the molar mass of carbon is $12 \text{ g/mol}$. (in $\text{ g/mol}$)

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