An element X has an atomic weight of 40 and a valency of 2. What is its equivalent weight?

Hydrogen peroxide in aqueous solution decomposes on warming to give oxygen according to the equation, $2{{\rm{H}}_2}{{\rm{O}}_2}\left( {aq} \right) o 2{{\rm{H}}_2}{\rm{O}}\left( l \right) + {{\rm{O}}_2}\left( {\rm{g}} \right)$ under conditions where one mole of gas occupies 24 ${\rm{d}}{{\rm{m}}^3},100{\rm{c}}{{\rm{m}}^3}$ of $XM$ solution of ${{\rm{H}}_2}{{\rm{O}}_2}$ produces 3 ${\rm{d}}{{\rm{m}}^3}$ of ${{\rm{O}}_2}$. Thus, $X$ is :

The equivalent weight of ${\rm{SnC}}{{\rm{l}}_2}$ in the reaction, ${\rm{SnC}}{{\rm{l}}_2} + {\rm{C}}{{\rm{l}}_2} o {\rm{SnC}}{{\rm{l}}_4}$ is :

Which of the following has the highest equivalent weight?

25 mL of 0.50 $M{{\rm{H}}_2}{{\rm{O}}_2}$ solution is added to 50 mL of 0.20 M $M{\rm{KMn}}{{\rm{O}}_4}$ in acidic solution. Which of the following statements is true?

The equivalent weight of ${\rm{MnS}}{{\rm{O}}_4}$ is half of its molecular weight when it is converted to :

What volume of ${{\rm{O}}_2}$ measured at standard conditions will be formed by the action of 100 mL of 0.5$N{\rm{KMn}}{{\rm{O}}_4}$ on hydrogen peroxide in an acidic solution? The skeleton equation for the reaction is,

${\rm{KMn}}{{\rm{O}}_4} + {{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4} + {{\rm{H}}_2}{{\rm{O}}_2} o {\rm{KHS}}{{\rm{O}}_4} + {\rm{MnS}}{{\rm{O}}_4} + {{\rm{H}}_2}{\rm{O}} + {{\rm{O}}_2}:$∶

The eq. wt. of ${\rm{KMn}}{{\rm{O}}_4}$ in the reaction, ${\rm{MnO}}_4^ - + {\rm{M}}{{\rm{n}}^{2 + }} + {{\rm{H}}_2}{\rm{O}} o {\rm{Mn}}{{\rm{O}}_2} + {{\rm{H}}^ + }$ (unbalanced) is :

56g of CO contains (NA = Avogadro’s No.)

The equivalent weight of sulfuric acid ($H_2SO_4$) is:

Mass ratio of $N{H_3}\,and{\rm{ }}C{O_2}$ for maximum product formation as per reaction : $2N{H_3} + C{O_2} o N{H_2}COON{H_4}$