Question

Question #81c72

Answer 1

Yes, the reaction is spontaneous.

Explanation:

We can answer this question by examining the standard reduction potentials for the half-reactions.

`color(white)(mmmmmmmmmmmmmmmmmmmmmmmmmmmml) E^@"/V"`
`2×["MnO"_4^"-" + 8"H"^"+" + 5"e"^"-" → "Mn"^"2+" + 4"H"_2"O"]; color(white)(mmmmmml)"+1.51"`
`5×["H"_2"C"_2"O"_4 → "2CO"_2 + "2H"^"+" + "2e"^"-"]; color(white)(mmmmmmmmmll)"+0.49"`
`2"MnO"_4^"-" + 5"H"_2"C"_2"O"_4 +"6H"^"+" → 2"Mn"^"2+" + 10"CO"_2 +8"H"_2"O"; "+2.00"`

The condition for spontaneity is that `ΔG < 0`.

`ΔG^@ = -nFE^@`

Since `E^@ > 0, ΔG^@ < 0`, and the reaction is spontaneous.