Enter the balanced chemical equation includingstates that describes the electroc

Question

Enter the balanced chemical equation includingstates that describes the electrochemical cell that is representedby the cell notation as shown.

Pt(s) l Cr3+(aq),Cr2O72-(aq), H+(aq) llH+(aq) l O2(g) l H2O(l) lPt(s)
St. Red. Pot. (V) Cr2O72-/Cr3+ +1.33 O2/H2O +1.23 Enter the balanced chemical equation includingstates that describes the electrochemical cell that is representedby the cell notation as shown.

Pt(s) l Cr3+(aq),Cr2O72-(aq), H+(aq) llH+(aq) l O2(g) l H2O(l) lPt(s)
St. Red. Pot. (V) Cr2O72-/Cr3+ +1.33 O2/H2O +1.23

Explanation / Answer

We Know that :     Oxidation half cell Reaction :      H2O (l)  --------> O2 (g) + 2e      Reduction half cell Reaction:         Cr2O7-2 (aq.) + 6e  ------> Cr+3 (aq.)       Net Cell Reaction :          3H2O (l) + Cr2O7-2 (aq.)  ---------> 3 O2 (g) + Cr+3 (aq.)          E0cell   = E0cathode - E0anode                       = + 1.33 V - ( + 1.23 ) V                         = + 0.10 V                       = + 1.33 V - ( + 1.23 ) V                         = + 0.10 V

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