The ΔG° r×n is gven as - 1059.42 KJ
The chemical equation is given as :
[tex]6Cr{2}^{+} + Cr{2}O{7}^{2-} + 14H^{+} -------- > 8Cr^{3+} + 7HO{2}[/tex]
ΔG r×n = - nFEcell
Ecell = Eoxidation + Ereduction
Eoxidation = -Ereduction =-(-0.50V) = 0.50 V
Ereduction = 1.33 V
Ecell = 0.50 V + 1.33 V
= 1.83 V
now, putting the value in formula
ΔGr×n = -nFEcell
where , n= 6 , f = faraday's constant = 96485 C/mol, Ecell = 1.83 V
therefore, ΔG r×n = - 6× 96487 × 1.83
= -1059.42 KJ
Now, ΔG°r×n = ΔG + RTlnQ
for standard condition Q = 1
hence ΔG°r×n = - 1059.42 KJ
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