Question

What is the equivalent weight of ${H_2}{O_2}$ in a decomposition reaction?

Answer 1

Hint: In a decomposition reaction a compound is broken down into two or more products. ${H_2}{O_2}$ is generally stored in dark containers. Otherwise it will decompose naturally in light and warm temperatures.

Complete answer:
Equivalent weight of any substance is the ratio of its molecular weight by the valence electron present in it that is the number of electrons transferred per mole. Here ${H_2}{O_2}$ is decomposed as
$2{H_2}{O_2} \to {O_2} + 2{H_2}O$
The number of electrons transferred per mole is $n = \dfrac{2}{2}$$ = 1$
The molecular mass of ${H_2}{O_2}$ is $H = 1 \times 2$$ = 2$ and $O = 16 \times 2 = 32$ giving a total of $34.01$
Molecular mass $MM$$ = 34.01$
Therefore molecular weight of ${H_2}{O_2}$ is $ = \dfrac{{MM}}{n}$$ = $ $\dfrac{{34.01}}{1} = 34.01$$g$.

Note:
Equivalent weight of a substance depends upon the reaction occurred. Equivalent weight can be used to calculate the normality of any substance. Decomposition reactions are used to extract metals from their ores.