Question

how many columbs of electricity areforthe following reduction process.1:1mole of Ag+.2:1 mole of Mno4-Mn2+​

Answer 1

Answer:

Explanation:

1. Formula required charge n × F

n = difference of charge on ions    

F is constant and equal to 96487 Coulombs

Here n = 3

Hence required charge = 3 × 96487 Coulombs

                                 = 289461 Coulombs

                                 = 2.89  ×10 –5 Coulombs

2. Charge on Mn in MnO4–

Charge on Oxygen is – 2

Mn + 4O     = – 1

Mn +4(–2)   = – 1

Mn              = +7

So our reaction is

MN7+  → Mn2+

n = 7– 2  = 5  

Required charge will  = 5 × 96487 Coulombs

= 482435 Coulombs

= 4.82 × 105 Coulombs

I'm not sure tho :/