Home
Class 12
CHEMISTRY
When 0.1 mol MnO(4)^(2-) is oxidized the...

When `0.1 mol MnO_(4)^(2-)` is oxidized the quantity of electricity required to completely oxidize `MnO_(4)^(2-)` to `MnO_(4)^(-)` is

A

`2xx96500 C`

B

`9650" C "`

C

`96.50" C "`

D

`96500"C"`

Text Solution

Verified by Experts

The correct Answer is:
B
(b) `underset(1" mol")(MnO_(4))^(-) to (MnO_(4))^(-)+underset(1F)e^(-)`
Electricity needed to oxidise 1 mole of `MnO_(4)^(-)` ions =1F.
Electricity needed to oxidise 0.1 mole of `MnO_(4)^(-)` ions =0.1 F =9650 C
Promotional Banner

Topper's Solved these Questions

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise COMPLETION QUESTION|2 Videos

  • ALCOHOLS AND PHENOLS

    DINESH PUBLICATION|Exercise NCERT In-Text Questions|9 Videos

  • ALDEHYDES AND KETONES

    DINESH PUBLICATION|Exercise Interger|5 Videos

Similar Questions

Explore conceptually related problems

The quantity of electricity required to reduce 0.5 mole of (MnO_(4))^(1-) to Mn^(2+) is

The quantity of electricity requried to reduce 0.05 mol of MnO_(4)^(-) to Mn^(2+) in acidic medium would be

What is best reagent to convert MnO_(4)^(2-) to MnO_(4)^(-) ?