What is the approximate volume (in mL) of 10 vol `H_(2)O_(2)` solution that will react completely with 1 L of 0.02 `M KMnO_(4)` solution in acidic medium?

Options

A. 56.05
B. 113.5
C. 90.8
D. 75.75

Answer

A

Explanation

The balanced equation between the reaction of `KMnO_(4)` and `H_(2)O_(2)` in acidic medium is as follows :
`2KMnO_(4)+5H_(2)O_(2)+3H_(2)SO_(4) rarr 5O_(2)+2MnSO_(4)+K_(2)SO_(4)+8H_(2)O`
thus, 2 mole of `KMnO_(4) equiv 5` moles of
`H_(2)O_(2) equiv 5` moles of `O_(2)(g)` at STP.
According to above relation:
34 g of `H_(2)O_(2)` will give `=11.2 L` of `O_(2)` at STP.
`:. (34 xx 5)`, i.e. 170 g of `H_(2)O_(2)` will give `=(11.2xx170)/34`
`=56 L`
`:' 1 L` of `H_(2)O_(2)` give 10 L of `O_(2)` at STP.
`:.` 1 mL of `H_(2)O_(2)` give 10 mL of `O_(2)` at STP.
and 56 mL of `H_(2)O_(2)` will give 560 mL of `O_(2)`
`:.` Volume of `H_(2)O_(2)=56` mL and (a) is the correct answer.