Question

BALANCING NET IONIC EQUATIONS!

Answer 1

\[H ^{+}+MnO _{4}+Fe ^{2+} \rightarrow Mn ^{2+}+Fe ^{3+}+H _{2}O\]

Answer 2

i have the right answer I just don't understand how

Answer 3

@aaronq

Answer 4

what exactly dont you understand?

Answer 5

why the balanced equations gives you five iron ions on each side?

Answer 6

the charge on \(MnO_4\) is -1. So it should actually be written: \(MnO_4^-\)

The reaction is actually a redox reaction, where Mn(VII) gains electrons to Mn(II)

this means it gained 5 electrons, these came from the iron atom.

\(Fe^{2+}\) changes to \(Fe^{3+}\), so each iron atom loses 1 electron.

Therefore you need 5 of them to balance the electron transfer.

Answer 7

how do we know they came from the iron ion

Answer 8

because in the equation the iron was oxidized. Look at the charges on them