Electrochemistry chem 5! help

(c) The cell represented below was set up under standard conditions.
Pt|Fe2+(aq), Fe3+(aq)||Tl3+(aq),Tl+(aq)|Pt Cell e.m.f. = + 0.48 V

(i) Deduce the standard electrode potential for the following half-reaction.
Tl3+(aq) + 2e– → Tl+(aq)
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(ii) Write an equation for the spontaneous cell reaction.
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Hi everyone i did the Q did it well - apart from spontaneous reaction i got 2fe3+ + Tl3+ ====) 2Fe2+ + Tl+

This was by using the anti-clockwise rule = however - the real answer for the Q was

Tl3+ + 2 Fe2+ ===) 2Fe3+ + T1+

Need an explanation why thanks!

Forget the anticlockwise "rule". Examiners can throw in a spanner by writing the list in a different order.

Spontaneous reaction requires that E_{(reduced half-equation)} - E_{(oxidised half-equation)} = positive value

Mnemonic E = E(red-ox)

i think there some information is missing there

i think there some information is missing there