Question

What are the appropriate balanced half-reactions for the following reaction, which is carried out in an acidic solution: I− + IO3− arrow I2 ?

I− arrow I2 (oxidized) and IO3 arrow I2 (reduced)

IO3 arrow I2 (oxidized) and I− arrow I2 (reduced)

2 I− arrow I2 + 2 e− (oxidized) and 2 IO3− + 2 e− arrow I2 (reduced)

2 I− arrow I2 + 2 e− (oxidized) and 2 IO3− + 10 e− arrow I2 (reduced)

Answer 1

please help!

Answer 2

What are the oxidation states/numbers for each of the atoms in the equation?

\( \huge \underbrace{I^−}_{-1} + \underbrace{IO_3^-}_{ (+5)(-2)} \leftrightharpoons \underbrace{I_2}_0\)

Oxidation: \(\huge 2~I^-\rightarrow I_2+2e\)

Reduction: \(\huge 2 ~IO_3^-+10e\rightarrow I_2\)

Answer 3

positive number

Answer 4

what do you mean?

Answer 5

im not sure im lost

Answer 6

@aaronq