Question

Identify each of these reactions as being spontaneous or nonspontaneous.

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Answer 1

I can’t view the images you uploaded. Please either paste the three reactions (including the ΔH and ΔS values or the temperature, or the standard cell potentials if they are electrochemical reactions), or re-upload the images as text.

If you want to decide spontaneity yourself, here’s how:

- For thermochemical reactions: use Gibbs free energy ΔG = ΔH − TΔS.
- If ΔG < 0 the reaction is spontaneous under the given conditions.
- If ΔG > 0 it is nonspontaneous.
- If ΔG = 0 it is at equilibrium.
- Special cases:
- ΔH < 0 and ΔS > 0 → ΔG always < 0 (spontaneous at all T).
- ΔH > 0 and ΔS < 0 → ΔG always > 0 (nonspontaneous at all T).
- ΔH < 0 and ΔS < 0 → spontaneous at low T (when T < ΔH/ΔS).
- ΔH > 0 and ΔS > 0 → spontaneous at high T (when T > ΔH/ΔS).

- For electrochemical reactions given standard potentials: calculate ΔG° = −n F E°cell.
- If E°cell > 0 → ΔG° < 0 → spontaneous under standard conditions.
- If E°cell < 0 → nonspontaneous under standard conditions.

Send the reaction details (ΔH, ΔS, T, or E° values) and I’ll classify each one and show the calculation.