Question

HELLO FRIENDS

Give reaction

When iron nails are placed in zinc sulphate??​

Answer 1

Answer:

$reaction$

Nothing happens at normal temperatures, because zinc is more reactive than iron, so iron will not displace the zinc from the zinc sulfate. However, if you crank the temperature to T ≥ 200C, then you can force a reaction:

ZnSO4•7H2O + Fe = FeSO4•4H2O + 3H2O(g) + Zn T ≥ 200C

Change in Free Energy: ΔG(200C) = -1.9kJ (negative, so the reaction runs)

Change in Enthalpy: ΔH(200C) = +229.8kJ (positive, so the reaction is endothermic)

Answer 2

Explanation:

reaction

Nothing happens at normal temperatures, because zinc is more reactive than iron, so iron will not displace the zinc from the zinc sulfate. However, if you crank the temperature to T ≥ 200C, then you can force a reaction:

ZnSO4•7H2O + Fe = FeSO4•4H2O + 3H2O(g) + Zn T ≥ 200C

Change in Free Energy: ΔG(200C) = -1.9kJ (negative, so the reaction runs)

Change in Enthalpy: ΔH(200C) = +229.8kJ (positive, so the reaction is endothermic)