Chemistry Alevel Question
In a test, aqueous iron(III) ions are reduced to aqueous iron(II) ions by iodide ions.
This reaction could be used to provide electrical energy in a cell.
(a) The standard electrode potential for the reduction of iron(III) ions into iron(II) ions can be measured by connecting a suitable electrode to a standard hydrogen electrode.
Draw a clearly labelled diagram to show the components and reagents, including their concentrations, in this Fe(III)/Fe(II) electrode.
Do not draw the salt bridge or the standard hydrogen electrode.
(3)
This reaction could be used to provide electrical energy in a cell.
(a) The standard electrode potential for the reduction of iron(III) ions into iron(II) ions can be measured by connecting a suitable electrode to a standard hydrogen electrode.
Draw a clearly labelled diagram to show the components and reagents, including their concentrations, in this Fe(III)/Fe(II) electrode.
Do not draw the salt bridge or the standard hydrogen electrode.
(3)
Reply 1
Original post
by fruitless-pointIn a test, aqueous iron(III) ions are reduced to aqueous iron(II) ions by iodide ions.
This reaction could be used to provide electrical energy in a cell.
(a) The standard electrode potential for the reduction of iron(III) ions into iron(II) ions can be measured by connecting a suitable electrode to a standard hydrogen electrode.
Draw a clearly labelled diagram to show the components and reagents, including their concentrations, in this Fe(III)/Fe(II) electrode.
Do not draw the salt bridge or the standard hydrogen electrode.
(3)
This reaction could be used to provide electrical energy in a cell.
(a) The standard electrode potential for the reduction of iron(III) ions into iron(II) ions can be measured by connecting a suitable electrode to a standard hydrogen electrode.
Draw a clearly labelled diagram to show the components and reagents, including their concentrations, in this Fe(III)/Fe(II) electrode.
Do not draw the salt bridge or the standard hydrogen electrode.
(3)
Honestly, I’d just draw a beaker containing a solution with an electrode sticking into it (this can be just a rod for simplicity, though in practice it’s not) then draw a wire connecting the electrode to a voltmeter.
As for the labels, we’re considering the Fe^3+ / Fe^2+ system. Because this is a redox equilibrium between aqueous ions and not a solid and some other species, it means the electrode must be made of Pt (so label the electrode with “platinum electrode” or similar - for future reference, it may be worth looking up what a platinum black electrode looks like if you wish to draw a more accurate diagram in future). We can also say with certainty that the solution must contain 1.00 mol dm^-3 Fe^2+ and 1.00 mol dm^-3 Fe^3+ (since standard conditions at A level implies the concentrations of all ions involved are 1 mol dm^-3 and we have identified the redox system as involving both iron(II) and iron(III) ions).
I’d also make sure to note that the temperature is 298 K. You could also state the pressure is 100 kPa, but since there are no gases involved, this is irrelevant.
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