Determine whether the reaction given below would be spontaneous or not. JUSTIFY your answer.
Fe2+ (aq) + Al (s) → Al3+(aq) + Fe (s)
This is done the same way a the Sn/Pb problem. Look up the activity series of metals.Post your work if you get stuck.
Would it be yes? My reason: Aluminum is on a higher level of activity than copper. Am I correct?
You are both correct and incorrect. Yes, the reaction is spontaneous because is above IRON(where did you get copper---or did you think Fe^2+ was copper) in the activity series. The symbol, Fe, from ferrum, is iron and Fe^2+ is ferrous or Fe(II).
To determine whether a reaction is spontaneous or not, we need to consider the thermodynamic factors involved, specifically the standard Gibbs free energy change (ΔG°).
The Gibbs free energy change is calculated using the equation: ΔG° = ΔH° - TΔS°.
- ΔH° represents the change in enthalpy (heat) of the reaction.
- T is the temperature in Kelvin.
- ΔS° is the change in entropy (disorder) of the system.
For a reaction to be spontaneous, the ΔG° should be negative, indicating that the reaction will occur spontaneously without the need for external input.
To determine ΔG° for the given reaction, we need to know the standard enthalpies of formation (ΔH°f) and standard entropies (ΔS°) of each species involved.
Once we have these values, we can calculate ΔG° using the equation above and assess whether the reaction is spontaneous or not.
Note: Unfortunately, as an AI text-based bot, I don't have access to real-time data like standard enthalpies of formation and standard entropies. However, you can find these values in thermodynamic tables or online databases. Once you have them, you can follow the steps above to calculate ΔG° and determine if the reaction is spontaneous or not.